LIBRARY OF CONGRESS. 

@]^ap ©op^risi^t 1 0- 

Slielf..Jia/fh 



UNITED STATES OF AMEKICA. 



1892 
COPYRIGHTED BY GEORGE WAHR. 



DIRECTIONS 



LABORATORY WORK 



URINE ANALYSIS 



FOR THE USE OF 



THE MEDICAL CLASSES 



UNIVERSITY OF MICHIGAN. 



/ 



FREDERICK &. :isrO^^Y, Sc. 33., IVX. 13., 

ASSISTANT PROFESSOR OF HYGIENE AND PHYSIOT-OGICAL CHEMISTRY. 



GEORGE WAHR, 

PUBLISHER AND BOOKSELLER, 
ANN ARBOR, MICH. 





l»( 



A 



THE COURIER OFFICE, PRINTERS. 



PART I. 



NORMAL m mmiki constituents of the urine. 



Preliminary Examination of the Urine. 



Examine under the microscope the following acci- 
dental constituents and note the characteristics of each : 

The diflferent varieties of starches. 

The textile fibres as cotton, hnen, silk and wool. 

Hair, epithelial cells and salivary corpuscles in saliva, and 

shreds of muscle. 
Tallow and lard crystals. Fatty globules in milk. 
Bacteria, yeast cells and filaments of moulds. 
Epithelium of the urinary passages. 

Behavior of normal urine with reagents. 

(1) Test the reaction with litmus-paper. What is it? 

(2) Heat some urine with a strong acid as HCl, HNO3, or H2SO4. 

Observe the peculiar odor that is emitted and the change 
in color. 

(3) Concentrate some urine in a small dish on the water bath, 

ignite and test the residue by means of a platinum wire and 
flame for potassium and sodium. 

(4) Add a few drops of oxalic acid or ammonium oxalate solution 

— calcium oxalate is thrown down. Examine its form under 
the microscope and test its solubility with acetic and hydro" 
chloric acids. 

(5) To some urine acidified with nitric acid, add a few drops of 

silver nitrate solution. AVhat is the nature of the precipi- 
tate ? Test its solubility with ammonium hydrate and with 
nitric acid. 



4 URINE ANALYSIS. 

(6) To some urine acidified with hydrochloric acid, add barium 

chloride. What does the precipitate indicate? Test its 
solubility in acids. 

(7) To some urine add uranium acetate solution. The yellowish 

white precipitate is uranium phosphate. Test its solubility 
in mineral acids, and in acetic acid. 

(8) Add a few drops of ferric chloride to some urine. What does 

the precipitate consist of? 

(9) Heat some of the urine in a test-tube. If strongly acid no 

change results, but if it is feebly acid or neutral the phos- 
phate of calcium is precipitated. Why? Write the formula 
of this salt. To a portion of the urine with this precipitate 
add nitric acid; cool another portion. What is the result? 

(10) To some urine add ammonium hydrate, ammonium magne- 

sium phosphate and calcium phosphate are thrown down. 
When the precipitate subsides examine it under the micro- 
scope. What is the form of the calcium phosphate? What 
is the form of the crystals of the ammonium magnesium 
phosphate? To a portion of the precipitate add acetic acid, 
to another portion hydrochloric acid. Note the result. 

(11) Render some urine alkaline with sodium or potassium hy- 

drate. The phosphates of calcium and magnesium are 
precipitated. Examine the precipitate under the micro- 
scope ; then test its solubility in acetic and hydrochloric 
acid. What are the results? 

(12) Add a few drops of mercuric nitrate solution to some urine. 

Observe that the precipitate formed by the first drop redis- 
solves on shaking ; that when an excess is added the pre- 
cipitate is permanent. To a portion of the precipitate add 
some sodium chloride solution ; to anotlier portion add nitric 
acid. Note the result. The precipitate contains urea. 

(13) To about 100 c. c. of the urine in a beaker add about 10 c. c. 

of hydrochloric acid and then set aside for 24 hours. The 
slight precipitate of reddish crystals consist of uric acid. 
Examine under the microscope. 

(14) Boil some urine with Fehliug's solution. What is the result? 

(15) Add a few drops of picric acid solution to some urine. Note 

the presence or absence of a precipitate. 

(16) To some urine add acetic acid, then a few drops of potassium 

ferrocyanide. Examine the same as under 15. 

(17) Heat some urine with Millon's reagent. 



PROPERTIES AND REACTIONS 



THE URINE CONSTITUENTS, NORMAL AND ABNORMAL. 



I 

UREA, CH,N,0 = CO. 

I 



■2 

1. Preparation from the urine: — Concentrate about 
500 c. c. of urine on a water-bath to a thin syrup ; cool this 
by immersion in ice-water and then add, at the same time 
stirring well, about three times its volume of strong nitric 
acid (1.3 specific gravity) which previously has been 
boiled to expel nitrous acid and then cooled to 0°. Allow 
the mixture to stand several hours at a low temperature 
— O" is best. Transfer the crystalline mass of urea nitrate 
which separates out to an asbestos filter (glass wool or 
sand), wash several times with small amounts of ice-cold, 
pure concentrated nitric acid, then dissolve in the smallest 
possible amount of hot water and again precipitate with 
concentrated nitric acid. Drain the crystals now obtained 
again on a filter, dissolve in hot water and decolor the solu- 
tion, if necessary, by addition of chlorine water or by a 
small amount of potassium chlorate, then treat with a 
small quantity of pure barium carbonate until efi'ervesence 
ceases and the solution reacts neutral. Evaporate on a 
water- bath to dryness, pulverize the residue and extract 
it repeatedly with cold absolute alcohol whereby the urea 
is dissolved and the barium salts are left behind. Filter 
and if necessary decolor the alcoholic filtrate by boiling 



6 URINE ANALYSIS. 

with animal charcoal, then concentrate to crystallization 
and set aside for crystals to form. 
Write out equations for 

1) Urea + nitric acid = 

2) Urea nitrate + barium carbonate = 

2. Synthetic prepo,ration:—^\\h up in a mortar 10 g:. 
of thoroughly dehydrated p-otassium ferrocyanide with 
3.75 g. of anhydrous potassium carbonate, transjer to an 
iron crucible or sand bath (2^-3 in. dism.), cover and 
heat over a Bunsen burner till perfect fusion results. To 
the somewhat cooled but still fluid mass add slowly and in 
small quantities 18.74 g. of well dried red lead, then heat 
for about ten minutes, at times stirring thoroughly with 
a glass rod, and finally pour the mass out on an iron 
plate. Pulverize the cooled mass and dissolve in about 21 
c. c. of water ; filter the solution of potassium cyanate thus 
obtained directly into an evaporating dish containing a 
solution of lO g. of ammonium sulphate in about 15 c. c. 
water. The potassium cj^anate is converted into ammo- 
nium cyanate. Evaporate the combined aqueous solution 
on a w^ater-bath to dryness. As a result of the heating the 
ammonium cyanate undergoes molecular transposition 
and becomes converted into its isomer— urea or carbamide. 
Extract the residue several times with warm absolute alco- 
hol, filter and evaporate the combined alcoholic filtrates 
on a water- bath almost to dryness, then set aside to crys 
tallize. Purify, if necessary by re-crystallizing several 
times from alcohol. 

Write out the equations representing the three stages 
in the above i)rocess. 

1) 4K4Fe(CN)6+4K2C03 + 5Pb30,= 

2) 2CNOKH-(NH,)2SO,= 

3) GN.0NH4= 

Why do we add potassium carbonate ? Why red lead ? 
Write equations showing the change that takes place 



THE URINE CONSTITUENTS, 7 

when potassium ferrocyanide is heated by itself ; when it 
is heated with potassium carbonate. 

iSynthetic preparation (Yolhard, Ann. 259^ 377): — 
Dissolve 3.9 g. of potassium cyanide and 1 g. of potassium 
hydrate in 100 c. c. of water, and add slowly a solution of 
6.3 g. of potassium permanganate in 100 c. c. of water ; 
keep the temperature below 17°. Now add 10 g. of am- 
monium sulphate and warm ; then filter off the manganese 
dioxide, evaporate filtrate to dryness and extract the resi- 
due with 95 per cent, alcohol, concentrate the alcoholic 
solution to crystallization. To remove traces of ammo- 
nium chloride dissolve the urea in a little water, add some 
barium carbonate, evaporate and extract the residue with 
absolute alcohol. 

Why is potassium permanganate used in this method ? 

Write the equation to represent the first stage. 
KGN + KMnO, + KOH= 

Properties of Urea. 

Determine the melting-point of the urea furnished by 
the laboratory ; that obtained from the urine and that pre- 
pared synthetically. What is the result ? 

The determination is made as follows : Heat a test- 
tube or a piece of soft glass tubing in a blast-lamp and 
rapidly draw apart. The narrow tube thus obtained is 
cut up into pieces about five inches long, each of these 
fused in the middle yields two tubes which are used in 
making the determination. Fill one of these tubes, sealed 
at one end, to a height of ^-^ inch- with the substance^ 
then fasten this by means of a small rubber band cut from 
a piece of rubber tubing, to a thermometer so that the 
sealed end of the tube is on a level with the end of the 
bulb of the thermometer. Suspend the thermometer 
with the attached tube in a beaker of about 100 c. c. 
capacity, containing enough sulphuric acid to clear the 
substance in the tube. Now heat with a small flame, stir- 
ring constantly, till the substance begins to melt. This is 
the melting-point; note the temperature. 



b URINE ANALYSIS. 

Ascertain the taste of a specimen of pure urea ? 
What is it like? 

Examine the crystals of urea under the microscope; 
recrystallize if necessary. Sketch the form of the crystals 
observed. 

Test the solubility of the urea in water, alcohol and 
ether. 

Salts of Urea. 

Urea nitrate, COfNHJ^.HNOs.— To about \ c. c. of 
concentrated urea solution or to some urine concentrated 
to about one-third, add an excess of strong nitric acid 
(free from nitrous acid — why?) If the precipit?te which 
forms does not show distinct crystals, redissolve by aid of 
heat and pour the contents of the test-tube out into a 
watch-glass. Examine the crystalline form under the 
microscope — sketch the same. Test the solubility of the 
crystals in water, alcohol and ether. 

Observe the formation of the crystals directly under 
the microscope, as follows : Place on a slide a drop or so 
of the urea solution, cover and apply a drop of nitric acid 
at the edge. 

Urea (^eZ^aZtxz^e, 2C0(NH Jg.U^CgO^.— To about ^ c. c. 
of concentrated urea solution add some concentrated 
oxalic acid solution. Redissolve the precipitate which 
forms by the application of gentle heat and pour the solu- 
tion into a watch-glass. Study and sketch the form of 
the crystals as observed under the microscope. Test the 
solubility the same as for nitrate. 

Observe the formation of the crystals directly under 
the microscope in the manner given for the nitrate. 

Mercuric Nitrate Compounds. 

1) 2CO(NHj3.Hg(N03),.HgO.— A compound hav- 
ing this composition is obtained when a nitric acid solu- 
tion of mercuric nitrate is added to a moderately dilute 
solution of urea nitrate. Examine the crusts which form 
on standing and sketch the crN stals. 



THE URINE CONSTITUENTS. ^ 

2) 2CO(Nn2)2.Hg(N03)3.2HgO. — This is formed 
when mercuric nitrate is added to a urea solution as long 
as a precipitate forms and this then set aside for some time 
at a temperature of 40-50°. Study and sketch the crys- 
tals which result. 

3) 2CO(NHj2.Hg(N03)3.3H:gO.— A compound pos- 
sessing this formula is formed when a faintly acid, approxi- 
mately 7 per cent, solution of mercuric nitrate is added to 
a 2 per cent, solution of urea. Note that the flocculent 
precipitate which forms becomes granular on standing. 
One of the methods for the quantitative estimation of 
urea depends upon the production of this precipitate. 

Treat a portion of the precipitate with nitric acid. 
Note the effect. 

Test another portion with salt solution. Observe the 
result and explain. 

Write the equation showing the formation of this 
precipitate. 

Calculate the ratio existing between the molecular 
weight of urea and of mercuric oxide from the composi- 
tion of the above precipitate. 

Reactions. 

Furfurol test: — Place a few crystals of urea in a por- 
celain dish, add 1-2 drops of a concentrated aqueous solu- 
tion of furfurol and 1-2 drops of concentrated hydrochloric 
acid — a faint yellow color which in a few minutes changes 
and a splendid purple appears. Intermediate tints of 
green, blue and violet may precede. (Schiff.) 

Benzoyl chloride test: — To about ^ c. c. of a concentra- 
ted aqueous solution of urea, add about 2 c. c. of sodium 
hydrate solution and ^ c. c. benzoyl chloride, then close the 
tube with a stopper and shake thoroughly. The tube be- 
comes hot and benzoyl urea, O (N H O Ce Hg) 3, forms. 
Test a specimen of urine (about 2 per cent. urea) in this 
way. Note the result and explain. Write the equation 
representing the reaction between urea and benzoyl chlo- 
ride (OOCI.Ce H5). 



10 URINE ANALYSIS. 

Bloxains test: — Acidulate a few crystals with hydro- 
chloric acid and evaporate in a (iish to dryness, then heat till 
white vapors (biuret) begin to be given off. Cool and 
test according to directions (4) on p. 11. 

Decompositions . 

1. Into avimonia and cyanate: — In the synthesis of 
urea it is prepared from ammonium cyanate and hence on 
decomposition it readily yields the compounds from which 
it is formed. Evaporate to dryness on the water-bath a 
few c. c. of a solution of urea to which some silver nitrate 
has been added — silver cyanate and ammonium nitrate 
form. Test a portion of the residue for ammonium by 
warming with potassium hydrate. Test another portion 
for silver cyanate as follows : Treat the residue with cold 
water and filter — silver cyanate is sparingly soluble in 
water and hence remains on the filter. To prove that this 
residue consists of silver cyanate, 1) to a portion add ammo- 
nium hydrate. What is the result? 2) To another portion 
add dilute nitric acid — note the eiFervescence. What is it 
due to ? Write an equation to represent the decomposition 
of urea in the presence of silver nitrate also an equation 
showing the action of nitric acid on silver cyanate. 

2. Into Bluret^G^^i^'dO^ : — Heat some urea in a test- 
tub« till it melts and keep it at that temperature until gas 
bubbles are given oif freely from the fused mass. Test the 
odor of the gas evolved. What is it? Now set the tube 
aside to cool, then dissolve in a little water and test as 
follows for biuret: To the aqueous solution add some 
potassium hydrate then a drop or less of a dilute copper 
sulphate solution. Note the bright pink color {Biuret re- 
action). What is the result when more copper sulphate 
is added? The conversion of urea into biuret can best be 
represented thus : 

'^'^"-NH, CO<NH, 

"= ^^ NH +NH3. 



THE URINE CONSTITUENTS. 11 

3. Into cyanuric acid, O3H3N3O3: — Heat some urea 
as just given under biuret till the gas ceases to be evolved 
and tlie contents solidify to a white chalky mass. Test 
this for cyanuric acid as follows : 

1.) Insoluble in cold, soluble in hot water from which 
it recrystallizes in prisms. 

2.) Dissolve a portion of the residue in cold concen- 
trated sodium hydrate, then heat. The sodium, salt which 
has formed recrystallizes in needles when its solution is 
heated. 

3.) Dissolve a portion of the residue in boiling water 
and add this to a dilute solution of ammonium cupric 
sulphate — a beautiful violet precipitate results. Avoid 
excess of ammonium hydrate or copper sulphate. 

4.) Dissolve a portion in a few drops of ammonium 
hydrate ; to one-half the solution add a drop of barium 
chloride solution — a crystalline precipitate forms ; to the 
remainder add a drop of a weak copper sulphate solution 
— a violet crystalline precipitate is produced. 

NH2 CO 

NH, _ >NH + 3 NH3. 

NH2 00 



NH; 
NH2 



yNH 

CO 



5.) Boil for some time an aqueous solution of urea 
in a test-tube in the mouth of which is placed a moist red 
litmus paper. What is the result and to what is it due ? 
Write the equation representing the decomposition of urea 
into ammonia and carbonic acid. 

6.) Heat some urea in a test-tube with potassium 
hydrate. Observe the .odor, and when the tube is cold 
acidulate with dilute hydrochloric acid — note the efferves- 
cence. To what is it due ? 

7.) To a few c. c. of concentrated urea solution in a 
test-tube add some nitrous acid, or about 2 c. c. of strongly 



12 URINE ANALYSIS. 

yellow colored nitric acid. What is the result ? Write an 
equation showing the action of nitrous acid on urea with 
carbonic acid, nitrogen and water as resulting products. 

8.) To some urea solution (or urine) add sodium hy- 
pobromite or hypochlorite. Note the effect. The reaction 
is represented by 

CO(NH3)8+3 NaBrO=3 NaBr+OO^-f N^ +2830. 

9.) To about 2 c. c. of permanganate of potash solu- 
tion, add some concentrated urea solution and then about 
^ c. c. of concentrated sulphuric acid. Note the eiferves- 
cence. 
2CO(NHJ, + Mn,07 = 2CO,-fN2 + 2NH3 + H,0 + 2Mn02 

Write this equation with symbol of potassium perman- 
ganate instead of MugO,. 

10.) Set aside some urine for several days. Then test 
the reaction — what is it, and to what is it due ? To a por- 
tion add some dilute acid — observe the effervescence. 

Write the equation showing the decomposition of urea 
into ammonium carbonate. 

Allow the litmus paper which was used to test the re- 
action to dry in the air. Notice that the original color 
returns. The color was due to volatile alkali — ammonia. 

Immerse a piece of red litmus paper in sodium hj^drate 
solution and then set aside to dry. 

Notice that the change in color remains permanent — 

due to fixed alkali. 

NH~C - NH 

CO I 

URIC ACID, C5H,N403 = ISTH-C CO. 

CO-NH 

Uric acid can be readily prepared (1) from the excre- 
ment of serpents, (2) from guano, (3) from uric acid calculi 
(4) from urine. 

Preparation from guano : — Boil some Peruvian guano 
repeatedly with milk of lime and water till the solution 
ceases to become colored. Then extract the insoluble 



THE URINE CONSTITUENTS. Id 

residue with boiling sodium carbonate till the filtrate on 
addition of hydrochloric acid ceases to give a precipitate. 
The combined filtrates are treated with sodium acetate 
and then hydrochloric acid added to a distinct acid reac- 
tion. The precipitate which consists of uric acid and 
guanine, is washed and then boiled with moderately dilute 
hydrochloric acid whereby the guanine is dissolved while 
the uric acid remains behind. 

Preparation from the urine. 

1.) To about 500 c. c. of normal filtered urine, free 
from albumin, add 10-15 c. c. of concentrated hydrochloric 
acid and set aside for 24-4:8 hours. The uric acid deposits in 
strongly colored crystals. Examine the crystals under the 
microscope and sketch the several forms observed. The 
deposit can be purified by dissolving in dilute alkali, then 
decoloring with animal charcoal and finally reprecipitating 
the uric acid with hydrochloric acid. 

2.) The best method for the isolation of uric acid, 
especially when the amount is small, is Ludwig's method, 
i e. precipitation with magnesia mixture and ammonia- 
cal silver nitrate. The precipitate is washed with ammo- 
nia water then decomposed by warming with potassium 
sulphide and filtered. The filtrate after addition of hydro- 
chloric acid is concentrated to a small volume, when the 
uric acid crystallizes. (See p. 63). 

Synthetic preparation of uric acid (Horbaczewski's 
method). 

Heat in a test-tube, in a small flame, 0.1-0.2 g. gly- 
cocoU with 1-2 g. of urea till the fused mass becomes solid- 
Avoid heating above 220°. The brownish-yellow mass 
thus obtained can be tested for uric acid with the murexide 
test (p. 16). To isolate the uric acid the contents of sev- 
eral tubes thus treated are dissolved in boiling water with 
addition of some ammonium hydrate and the filtrate 
treated with magnesia mixture and ammoniacal silver ni- 



14 URINE ANALYSIS. 

trate ; from the resulting precipitate uric acid is obtained 
as given under Ludwig's method (p. 63). 

The necessary glycocoll can be prepared from hippuric 
acid. (See p. 24.) 

The synthetic process can be represented by the 
equation : 

C2 H5 NO2 +3OH4 N2 0=C5 H4 N4 O3 -f 3NH3 +2H2 O. 

Properties of uric acid. 

Examine under the microscope the form of the crystals 
of the laboratory specimen and that obtained from the 
urine. 

Place a few crystals on a slide, add a drop of potas- 
sium hydrate solution and watch the solution of the crys- 
tals through the microscope. When dissolved apply a 
drop of concentrated acetic acid to the edge of the cover- 
glass, and again examine. What i.^ the result ? 

Test the solubility of the crystals in water, alcohol, 
ether, potassium hydrate, ammonium hydrate, hydrochlo- 
ric acid. 

Salts of uric acid. 

Sodium acid urate, O5 H3 NaN4 O3 : — To some uric acid 
in a test-tube add water and boil, then add sodium hydrate, 
drop by drop, till it dissolves. To the solution thus ob- 
tained add sodium bicai*bonate, or pass carbonic acid gas 
till it is almost neutral. Set aside over night to crystall- 
ize. Recrystallize if necessary from hot water and ex- 
amine the crystals under the microscope. Sketch a few 
of the same. What is the formula of the normal sodium 
urate ? 

Potassium acid urate, C5 H3 KN4 O3 , is prepared in the 
same manner as already given, using however, potassium 
hydrate instead of sodium hydrate. Examine and sketch 
the crystalline form. 

Ammonium acid urate, Cg Hg (NH4 )N4 Os :— This is 
readily prepared in the manner already given, by boiling 



THE URINE CONSTITUENTS. 15 

with ammonium hydrate. If the precipitate fails to 
dissolve and the solution is strongly ammoniacal, add water 
till complete solution results, then set aside to crystallize. 

Examine the crystals and compare with the preced- 
ing. 

Does the normal ammonium urate exist '^ 

Calcium urate, can be prepared in a similar manner 
as the preceding by adding calcium hydrate to the boiling 
mixture till the uric acid dissolves. On cooling the salt 
crystallizes. Examine as before. 

Sulphates of uric acid, as Cg H4 N4 O3 AB2 SO4 .—Add 
uric acid to some hot concentrated sulphuric acid as long 
as it dissolves. On cooling large transparent crystals sepa- 
rate which on the addition of water decompose into the 
constituents. 

Reactions. 

1.) To some uric acid add water, boil, then add 
ammonium hydrate, drop by drop, till it dissolves. Dilute 
with an equal volume of water, add hydrochloric acid to 
acid reaction and immediately after add a solution of 
phosphotungstic acid — a bright chocolate-brown granular 
precipitate appears. 

2.) To some uric acid dissolved as above, add picric 
acid — a voluminous yellow precipitate forms. — (Jaffe). 

3.) To uric acid dissolved and diluted as above, add 
ammoniacal silver nitrate. Note the result. Now add a 
little of a solution of a neutral salt as sodium chloride, 
ammonium sulphate, or better still magnesia mixture — a 
flocculent or gelatinous precipitate is at once thrown down. 
It is a compound of uric acid, silver and the base employed. 
What is magnesia mixture? 

4.) To some uric acid add water, boil and add a lew 
drops of sodium hydrate and a few drops of Fehling's solu- 
tion. On heating the white cuprous urate is thrown down. 
Allow the precipitate to subside, decant the supernatant 
fluid and add some new Fehling's solution and boil for 



16 URINE ANALYSIS. 

some time. The red cuprous oxide is gradually formed. 
(Compare with test for sugar p. 46). 

What is Fehling's solution? Write the formula of 
cuprous oxide. 

5.) Dissolve a few crystals of uric acid in a little so- 
dium hydrate, then pour the liquid upon a filter which 
previously has been moistened with a drop of silver nitrate 
solution — a yellowish to a brownish black stain indicates 
reduced silver. This is a very delicate test and is given 
by as little as 1-500 mg. uric acid. 

6.) Miirexide Test .-—Place a minute quantity of 
uric acid in an evaporating dish, add nitric acid and 
evaporate to dryness on the water-bath. A yellowish resi- 
due results which on contact with the vapors of ammonia 
turns to a beautiful pink or red (ammonium purpurate or 
murexide). Now add a drop of potassium hydrate. Note 
the change in color and the fact that this disappears in a 
short time on standing — distinction from the xanthine 
compound which in addition is more of a red color. 

The change that takes place in the above reaction is 
as follows: The uric acid is oxidized by the nitric acid to 
alloxantin which is a combination of alloxan and dialuric 

acid (C!0<^^~QQ> CH— OH Y Addition of ammonia 
converts the latter into dialuramide, 

CO<™zgg>GH-NH„ 

(uramil) which with alloxan yields purpuric acid. Excess 
of ammonia produces ammonium purpurate or murexide. 
(see formula p. 22). 

Why is it called murexide? Is purpuric acid known 
in the free state ? 

T.) Heat sharph^ some uric acid in a test-tube. It 
decomposes into ammonia, hydrocyanic acid (recognized 
by its peach-blossom odor), urea and cyanuric acid. 



THE URINE CONSTITUENTS. 17 

Decompositions. 

Uric acid on oxidation may yield three distinct 
groups of products. 

1.) In cold acid solution yields urea and alloxan — the 
alloxan group. 

2.) In warm acid solution yields parabanic acid — the 
parabanic group. 

3.) In neutral and alkaline yields allantoin — the 
allantoin group. 

I. ALLOXANTIN: CsH^N.O.+SH.O. 

To 5 g. of uric acid iii a small Erlenmeyer flask 
add 10 c. c. of concentrated hydrochloric acid (sp. gravity 
1.19) and 10 c. c. of water. Now add very slowl}^ and 
in small portions 1.5 g. of finely pulverized potassium 
chlorate. No chlorine or carbonic acid should be evolved. 
Nearly all the uric acid passes into solution as urea and 
alloxan, O4H2N2O4, which on reduction can readily be con- 
verted into alloxantin. For this purpose dilute the liquid 
with an equal volume of water, filter off the unchanged uric 
acid, and through the filtrate, returned to the flask, pass hy- 
drogen sulphide as long as a precipitate continues to form. 
Alloxantin is thrown out of solution mixed with free sul- 
phur. Set the flask aside over night in the cold. Then 
extract the alloxantin by heating several times with boil- 
ing water, and filter. Alloxantin crystallizes from the 
filtrate on cooling in colorless prismatic crystals. Filter 
off the crystals and dry between filter paper. 

Write out the following equations which represent the 
two stages in the process. 

C,H,N,03 + + H30 = 

Tests for Alloxantin. 

1). Examine the crystals under the microscope and 
sketch the form. 



18 URINE ANALYSIS. 

2.) To a few crystals of alloxantin in a porcelain dish 
add a drop of ammonium hydrate. Note the results. Then 
add a drop of potassium hydrate and observe the change if 
any. To what is this due? 

3.) Dissolve a few crystals of alloxantin in boiling 
water and add some barium hydrate solution. A violet- 
blue precipitate forms which on heating becomes white 
(due to formation of barium alloxanfcate and dialurate). 

4.) To an aqueous solution of alloxantin add some 
ammoniacal silver nitrate. What is the result and to 

what is it due ? 

NH— CO 

11. ALLOXAN: C.H.NgO, =00 CO 

NH-CO. 

A.) To the powdered alloxantin prepared as just given 
(about 2 g.) add about 4 c. c. of fuming nitric acid(1.50 sp. 
g.) and 2.5 c. c. of concentrated nitric acid (1.42 sp. g.). 
Rub up in a mortar or dish, then set aside in a stoppered 
test-tube for several days till a specimen of the crystals 
taken out dissolves readily and completely in water which 
occurs as soon as all the alloxantin has been converted 
into alloxan. When this is the case transfer the crystals 
to a porous porcelain plate (or asbestos filter) to dry, then 
place in a porcelain dish and heat on the water bath, stir- 
ring constantly, till the odor of nitric acid disappears. 
Recr3^stallize from a very small amount of hot water. 

The reaction is represented by the equation : 

C3H,N,0,-|HN03= 2C4H3N,04 + HNO,. 

Tests for Alloxan. 

1.) Study and sketch its crystalline form. How do 
the crystals behave on exposure to air ? 

2.) On boiling with barium hydrate it decomposes 
^CO^H 
intomesoxalic acid, CO and urea. Write out the equa- 
CO,H 



THE URINE CONSTITUENTS. l9 

tion employing graphic formulae. On warming with nitric 

NH— 00 

acid it is oxidizad to parabanic acid, 00 , and CO2 . 

NH— 00 

The former bv the action of the alkalies yields oxaluric acid, 

I POOT-T 

00 , which in turn decomposes into oxalic acid, , 

JSIH— 00— OOOH OOOH ' 

and urea. 

Write out the equations representing these three 
changes. 

4.) Formation of murexide — Dissolve a few crystals 
of alloxan in a little water in a dish, evaporate to dryness 
and add ammonium hydrate. 

5.) To an aqueous solution of alloxan add excess of 

baryta water — a white precipitate of barium alloxantate 

forms. 

NH-OH— NH 

III. ALLANTOIN: O.HeN.Oa = 00 j 

NH— 00 00 

NB, 
To 4 g. of uric acid stirred up in about 100 c. c. of water 
add sodium hydrate till it dissolves, and when cold add 
gradiijally 3g. of powdered potassium permanganate. As 
soon as aU the permanganate has been added and dissolved, 
filter. Acidulate the filtrate with acetic acid as soon as 
possible, then set aside in a cold place over night. Filter 
ofi" the crystals which form and wash with water ; combine 
the wash- water and filtrate, concentrate on the water bath 
to a small volume, then set aside over night. The crystals 
that form can be combined with those previously obtained 
and recrystallized from a small amount of hot water. 
The oxidation takes place according to the equation. 

O5H,N,O3 + H.O + O=0O2 + 04H6N,O3 
Write out the following equation in which potassium 
permanganate is used as above. 

05H,N403 + H.O + KMnO = 



20 URINE ANALYSIS. 

Properties of Allantoin. 

1.) Examine and sketch the crystalline form. 

2.) Test the solubility in water; also the reaction. 

3.) To an aqueous allantoin solution add a drop or so of 
silver nitrate solution. No precipitate forms, then add a 
drop of dilute ammonium hydrate when a white precipitate 
of allantoin-silver, C4HgAgN403 , forms. Test the solu- 
bility in ammonium hydrate and nitric acid ; also examine 
the precipitate under the microscope. 

4.) To some allantoin solution add mercuric nitrate 
when a white flocculent precipitate forms. Compare with 
the behavior of urea (p. 8). To the precipitate add ammon- 
ium hydrate and warm. Note the change and explain. 

5.) Allantoin, like urea, gives the furfurol test (p. 9), 
except that it comes slower and is'less intense. 

6.) It does not yield the murexide test. 

7.) On prolonged boiling with Fehling's solution it 
yields cuprous oxide. Compare with the uric acid (p. 15). 

8.) Dissolve some allantoin in a little potassium 
hydrate and divide the solution into two portions. To one 
add acetic acid— the allantoin is precipitated. Set the 
other portion aside for several days, then add acetic acid — 
no precipitate forms. The allantoin has been converted 
into allantoic acid, C4H8N4O4 . 

9.) On heating with acids, allantoin yields allanturic 

acid, C3H4N2O3, and urea, 

C,H;N403-fH,0-C3H4N,034-CO(NH,),. 

10.) Boil some allantoin with concentrated sodium 
hydrate till ammonia vapors are given off (what does this 
indicate ?) ; then acidulate with acetic acid, and add a few 
drops of calcium chloride solution. Test the precipitate 
with acetic and hydrochloric acids. What is it ? Alkalies 
yield the same products as acids, but on prolonged heating 
the allanturic acid decomposes into hydantoic and para- 
banic acids. The parabanic acid in turn is decomposed 
into oxalic acid and urea. 



THE URINE CONSTITUENTS. 21 

203H,N,O3 = CaHeN.Os + C3H,N30, . 

Hydantoinic acid. Parabanic acid. 

, C3H3N203+2HjO = H^OsO.+OOCNHJj . 

CKEATINIiNE,C4 H, N3 O = NH=0<JJ^^^7~~5o ' 

JN((JH3 )— CH2 

The following method of isolation can also be used for 
quantitative estimation (Neubauer's method):— 200-300 c.c. 
of urine are rendered alkaline with calcium hydrate and 
then calcium chloride is added to precipitate the phos- 
phates. Baryta mixture can be used to precipitate the 
phosphates. The precipitate is filtered off and washed ; the 
filtrate and wash-water are combined, slightly acidulated 
with acetic acid, and evaporated to a syrup. This while 
warm is mixed with 50 c.c. of 95-97^' alchohol and the mix- 
ture, transferred to a beaker, is covered and allowed to 
stand eight hours in the cold. The precipitate is then fil- 
tered off*, washed with alcohol, and the filtrate if necessary 
is concentrated to 50-60 c.c. When cold one-half a c. c, of a 
zinc chloride solution, of a specific gravity of 1.20 and free 
from acid, is added. The thoroughly stirred mixture is cov- 
ered and allowed tostand in a cold place for two to three 
days. The precipitateis collected ujjon a small weighed 
filter. The filtrate can be used to transfer all the crystals. 
These are then washed with a little alcohol till all the chlo- 
rides are removed and finally dried at 100° C. and weighed. 
100 parts of creatinine zinc chloride contains 62.42 parts of 
creatinine. From this compound the pure creatinine can 
be obtained by heating with lead hydrate. The solution is 
filtered, decolored with animal charcoal, evaporated to 
dryness and the residue extracted with strong alcohol 
(creatine remains undissolved). The alcoholic solution can 
be concentrated to crystallization and if need be the cays- 
talscan further be purified by recrystallization from water. 

XANTHINE COMPOUNDS. 

The following members of the group may be obtained 
from urine : Xanthine, hj^poxanthine, guanine, paraxan- 
thine and heteroxanthine. 



22 URINE ANALYSIS. 

Isolation. — The urine is treated with ammonia in ex- 
cess and precipitated with ammoniacal silver nitrate. The 
precipitate is then decomposed with hydrogen sulphide and 
filtered while boiling hot. The filtrate is evaporated to 
dryness and the residue treated with 8 % sulphuric acid 
whereby the xanthine compounds are dissolved while 
uric acid remains behind. The filtered liquid is treated 
with ammonia in excess and precipitated with ammoniacal 
silver nitrate. The different compounds can then be iso- 
lated by treatment with hot nitric acid of specific gravity 
1.1. For details of isolation, etc., see Yaughan andNovy— 
Ptomaines and Leucomaines pp. 314, 322. 



THE URINE CONSTITUENTS. 23 

Formulae of Uric Acid and its Chief Derivatives. 

NH— C— NH NH— CH— NH NH— CH NH NH— CH— OH 

CO I I CO I I CO I I CO I 

NH— C CO NH— CO CO NH2 COOH C NH— CO 
CO-NH NH2 NH2 



URIC ACID. ALLANTOIN. ALLANTOIC ACID. ALLANTURIC ACID. 

(Glyoxyl-diureM.) (Glyoxyl Urea.j 

C5H4N4O3.. CiHeN^Oa. C4HsN,04. CsH.N^Oa. 



NH— CO NH— CO NH— CO NH— CO 
CO CO CO CO CO CHOH CO CH 
NH— CO NH COOH NH— CO NH— CO 



ALLOXAN. A.LLOXANIC ACID. DIALURIC ACID. BARBITURIC ACID. 

(Mesoxalyl Urea ) (Tartrouyl Urea.) (Malonyl Urea.) 

C4 H2 N2 O4 . C4 H4 N2 O5 . C4 H4 N2 O4 . C4 H4 N2 O3 . 



Alloxantin (Alloxan + Dialurie Acid), Cg H4 N4 O7 . 
Purpuric Acid (Alloxan + Dialuramide), Cg H5 N5 Oe . 
Ammonium purpurate or murexide (Alloxan + Am- 
monium dialuramide), Cg H4 N5 Oe (NH4 ). 



NH— CO 


NH— CO 


NH— CH2 


NH— CO 


CO 


CO 


CO 


CO CH-NH, 


NH— CO 


iH2 COOH 


NH2 COOH 


NH— CO 



PARABANIC ACID. OXALURIC ACID. HYDANTOIC ACID. AMIDO-BARBITUR- 

IC ACID. 

(Oxalyl Urea.) (Uramil, Dialuramide.) 

C3 H2 N2 O3 . C3 H4 N2 O4 . C3 He N2 O3 . C4 H5 N3 O3 . 



24 URINE ANALYSIS. 

HIPPURIC ACID, Cg H9 NO3 = Ce H5 CO.NH.OH2.CO2 H. 
Preparation from the Urine. 

Boil I — 1 liter of urine (of the horse or cow) with excess 
of thin milk of lime ; filter while hot and concentrate the 
filtrate on a wire gauze to | — | the original volume. 
Cool and add excess of hydrochloric acid and set aside 
for 24 hours. Filter off the reddish crystals of hip- 
puric acid and dry them between filter paper. Dis- 
solve the crystals of crude hippuric acid in as little 
water as possible, filter; heat filtrate to boiling and pass 
chlorine gas till the color of the solution becomes pale yel- 
low. Then cool rapidly, filter and wash the crystals 
several times with cold water. Recrystallize from boiling 
water to which animal charcoal has been added. (Curtius). 
To purify the crystals boil again with milk of lime, filter 
and reprecipitate with hydrochloric acid. The crystals 
can be still further purified b}^ recrystallization and decol- 
oring with animal charcoal. 

Human urine can be employed if a dose or two of 
benzoic acid has previously been taken. 

Synthetic Preparation. 

To some glycocoll in a test-tube add a little water, then 
a few drops of sodium hydrate and about one c. c. of 
benzoyl chloride. Close the tube with a stopper and 
shake vigorously as long as the tube continues to become 
hot. Finally render strongly alkaline with sodium hydrate 
and shake until the odor of benzoyl chloride disappears. 
When cold acidulate with hydrochloric acid, add an equal 
volume of ether (petroleum ether is better) and thor- 
oughly shake up in order to extract the benzoic acid. 
Decant the ethereal layer into a clear porcelain dish and 
repeat the extraction as before. The aqueous solution 
with the insoluble hippuric acid is filtered, and the hip- 
puric acid washed slightly on the filter with cold water, 
then recrystallized from a small amount of boiling water 
(just sufficient to dissolve). 



THE URINE CONSTITUENTS. 25 

The ethereal solution on evaporation j^ields benzoic 
acid. 

The synthesis takes place according to the equation : 

COo H (JO2 H 

Properties of Hippurio Acid- 
Determine the melting-point. What is it ? 
Test (he solubility in alcoho], ether and water. 
Test the taste and reaction. 

Examine the crystalline form under the miscroscope. 
Carefully neutralize a solution of hippuric acid with 
sodium hydrate, and add a drop or two of neutral ferric 
chloride solution when the cream colored ferric salt is pre- 
cipitated. Test the solubility in hot water, hot alcohol 
and acids. 

Reactions. 

1.) Boil a few crystals of hippuric acid with some 
sodium hypobromite solution — a kermes-brown precipi- 
tate forms (distinction from benzoic acid). 

2.) Place some hippuric acid in a dish, add nitric 
acid and evaporate to dryness. Transfer the residue to a 
test-tube and heat in a Bunsen flame. Observe the odor of 
nitro-benzol (artificial oil of bitter almonds). 

3.) On moderate heating in a test-tube hippuric acid 
melts to an oily fluid which on cooling solidifies to 
a crystalline mass. On stronger heating the liquid becomes 
red, rises along the walls of the tube and yields a subli- 
mate of benzoic acid and the odor of hydrocyanic acid 
(peach-blossoms). 

4.) Place one gram of hippuric acid in a small 
Erlenmeyer flask, add about 10 c. c of dilute sulphuric 
acid (1-2), then insert a perforated stopper provided with 
an upright glass tube 12-18 inches in length (condensing 
tube). Heat the contents on a wire gauze at just below 
the boiling point for some hours. Observe the sublima- 
tion of crystals of benzoic acid. When the decomposition 



26 URINE ANALYSIS. 

is complete, cool, add about 25 c. c. water and filter oif the 
benzoic acid. Extract the filtrate with ether to remove 
the dissolved benzoic acid; then dilute the aqueous liquid 
with water and neutralize on the water-bath with barium 
carbonate. Filter, concentrate the filtrate on the water- 
bath almost to dryness, and set aside to allow the gly- 
cocoll to crystallize. 

Complete the equation : 

C.Hg. CO. NH. CHg. C03H+H30= 

Save the benzoic acid for subsequent tests. 

BENZOIC ACID, C,H603=C6H5.COOH. 

Preparation. 

This acid is obtained in the decomposition of hippuric 
acid^(see p. 25) and can be purified by recrystallization 
from hot water. 

Properties. 

1.) Examine the crystalline form as it is obtained 
(1) from hot water, (2) from ether. 

2.) Heat some benzoic acid in a test-tube, held 
vertically over the flame, — the acid sublimes in needles. 
Note the odor evolved. 

3.) Determine the melting point of the crystals. 

4.) Test the solubility in water, alcohol, and in ether. 

5.) To a solution of a salt of benzoic acid add 
neutral ferric chloride solution. To a portion of the 
brownish yellow precipitate which forms add ammonium 
hydrate — it di so Ives and ferric hydrate is thrown down 
instead. To another portion add hydrochloric acid and 
set aside over night. What is the result? 

6.) Place some benzoic acid in an evaporating dish, 
add nitric acid and evaporate over a flame to dryness ; 
then gently heat — the odor of nitrobenzol (artificial oil 
of bitter almonds) will be perceived. 

7.) With sodium hypobromite it gives no precipi- 
tate — distinction from hippuric acid. 

8.) Add a solution of benzoic acid or its salt to a 



THE URINE CONSTITUENTS. 27 

mixture of alcohol, barium chloride and ammonia. No 
precipitate forms — distinction from succinic acid. 

CO OH 
OXALIC ACID, C.H20,= | 

CO OH 

Preparation of Calcium oxalate. 

To about 200 c. c. of urine add a few drops of satu- 
rated oxalic acid solution, then set aside for twenty-four 
hours. Examine the sediment under the microscope for 
the characteristic octahedral crystals, and other forms. 

Properties of Calcium oxalate. 

1.) Examine and sketch the different forms of cal- 
cium oxalate. 

2.) Test the solubility in water, acetic acid, hydro- 
chloric acid. 

SULPHURIC ACID, H^SO,. 

To about 10 c. c. of urine in a test-tube add some 
acetic acid, then some barium chloride solution — barium 
sulphate is precipitated Now filter and to the filtrate add 
hydrochloric acid (1 c. c), boil for a few minutes, and set 
aside. A precipitate forms. What is it? Explain the 
reaction. 

The experiment shows that sulphuric acid exists in 
the urine in at least two forms — as ordinary sulphate, and 
as ether sulphuric acid salts. 

Write the equations. 

1.) BaCl3 + K3SO,= 

2.) Ce Hg.O. SO3. 0K+H30=KHS04 + 

Prepare and examine under the microscope crystals 
of calcium sulphate. 

Apart from the two forms of sulphuric acid mentioned 
above there are present in the urine substances as cj^stin, 
taurin, hyposulpliurous acid, sulphocyanic acid, etc., which 
contain sulphur in the unoxidized or incompletely oxid- 
ized conditions. These are spoken of as containing 



28 UEINE ANALYSIS. 

" neutral " sulphur, and can be detected and estimated 
in the following manner : — 

Filter off the barium sulphate precipitate which forms 
in the hydrochloric acid solution as described above and 
from the filtrate remove the barium by careful addition 
of sodium carbonate solution. Filter, evaporate the 
filtrate to dryness, and fuse the residue with pota&sium 
nitrate and hydrate. Dissolve the fused mass when cold 
in water, acidulate with hydrochloric acid and precipitate 
with barium chloride — the neutral sulphur has been oxid- 
ized to sulphuric acid. 

HYPOSULPHUROUS ACID, H-.S^Og. 

Make the following tests with a solution of sodium 
hyposulphite : — 

1.) Warm some of the solution with hydrochloric 
acid — notice the odor, and the cloudiness due to separa- 
tion of free sulphur. 

Complete the equation : — 

Na,S,03 + 2HCl= 

This test may be applied to a urine suspected of con- 
taining hyposulphurous acid, as that of a cat or dog — a 
milky appearance on standing is due to free sulphur. 

2.) To a few c. c. of the solution add a few drops of 
silver nitrate solution. The solution on standing becomes 
black from reduced silver. 

3.) Add 1 to 2 drops of neutral ferric chloride to some 
of the solution. What is the result ? 

4.) To some hyposulphite solution add barium chlo- 
ride, then alcohol — the difficultly soluble barium salt 
forms. 

POTASSIUM PHENOL SULPHATE. 
C^Hg.O. SOg. OK. 
Synthetic Preparation. 

Prepare first some potassium pyrosulphate as follows : 
To 10 g. of pulverized potassium sulphate in an evaporat- 
ing dish add 6 g. of concentrated sulphuric acid and warm 



THE URINE CONSTITUENTS. 29 

gently over a flame, stirring well, till the mass dissolves ; 
then gradually raise the heat till the mass remains in 
quiet fusion. Cool and pulverize. 

Now place in a flask 6 g. of potassium hydrate dis- 
solved in 8 to 9 c. c. of water and add 10 g. phenol. When 
all is dissolved, cool to 60-70° and add gradually and in 
small portions, agitating well, 12.5 g. of -the finely pul- 
verized potassium pyrosulphate. Keep the mixture at 
60-70°, with frequent shaking, for 8 to 10 hours ; then add 
about 50 c. c. of boilin.2; alcohol, shake thoroughly and 
filter while hot. The filtrate on cooling solidifies to 
a mass of bright plates of potassium phenol-sulphate. 
Recr^^stallize once or twice from boiling alcohol and 
finall}^ dry the crystals between filter paper or in desic- 
cator over sulphuric acid. 

The synthesis of this salt is shown by the equation: 

Ce Hs .OK-f .K2 So O, =C6 H5 .0. SO2 .OK4K2 SO4 . 

Reactions. 

1.) An aqueous solution of potassium phenol-sulphate 
is not precipitated by barium chloride even in presence of 
acetic acid. Why not? 

2.) To an aqueous solution of the salt add hydro- 
chloric acid and heat a few minutes, then add barium 
chloride. What is the result? Write the equation to 
represent the change. 

3.) In solutions of the salt test for phenol Avith 
bromine- water, ferric chloride, and Millon's reagent. 
What is the result? 

4.) Distil a solution of the same, acidulated with 
hydrochloric acid, and in the distillate test for phenol. 

Make the following tests for phenol : — 

1.) To a dilute solution of phenol add a drop of 
neutral ferric chloride solution — violet color. 

2.) To the phenol solution add bromine- water to a 
permanent yellow color — yellowish white precipitate of 
crystals of tribromphenol, Cq H2 61-3 OH. Examine under 
the microscope. 



30 URINE ANALYSIS. 

3.) To the phenol solution add some Millon's reagent 
and warm till precipitate dissolves — beautiful red color. 

Detection of phenol in the urine. 

To about 500 c. c. of horse's or cow's urme add 25 c. c. 
sulphuric acid and distil. Examine the distillate by the 
above tests for phenol (and cresol). 

INDOXYL, Og H, NO = Ce H4 <^- h^>C H. 

This occurs in the urine as potassium indoxyl sul- 
phate, Cs HgN. O, SO2 .OK, commonly known as indican. 

Jaffe's test for Indoxyl. 

To some urine in a test-tube add an equal volume of 
concentrated hydrochloric acid, a few c. c. of chloroform, 
then drop by drop a dilute solution of sodium (or calcium) 
hypochlorite. Shake after each addition. The chloroform 
gradually turns blue since the indoxyl has been oxidized 
to indigo-blue. 

2 Cs H, NO+20=Ci6HioN2 O, -f 2 H^ O. 

The same process may take place in alkaline urine in 
the presence of air in which case the indigo separates in 
stellate needles or plates. Gentle warming with ferric 
chloride and hydrochloric acid will also bring about the 
same result. 

Tests for Indol :— 

1.) The solution is colored red by nitric acid con- 
taining a trace of nitrous acid. 

2.) A pine splinter moistened with hydrochloric acid 
is colored red. 

3.) Examine a specimen of indol in the laboratory — 
note the odor. 

SKATOXYL. C9H9NO. 

The potassium salt of skatoxyl sulphuric acid, C9 Hs N. 
O. SO2 .OK, may occur in the urine. 
Skatoxyl itself is unknown. 



THE URINE CONSTITUENTS. 31 

Detection of Skatoxyl. 

1.) To the suspected urine add hydrochloric acid; 
if skatoxyl is present a dark red to violet color will 
appear. 

2.) Addition of nitric acid to the suspected urine will 
produce a cherry-red color if skatoxyl is present. 

3.) Urine containing much skatoxyl darkens like 
carbolic acid urine and later becomes reddish, then violet 
to black. 

Tests for Skatol :— 

1.) Does not give a red color with nitric acid which 
contains nitrous acid, but only a whitish cloud. 

2.) Does not color a pine splinter moistened with 
hydrochloric acid. 

3.) Note the odor of a specimen of skatol. 

PYROCATEOHIN, Ce H4 (OH)^ . 

This is ortho-dioxybenzole (1.2) and occurs in the 
urine as pyrocatechin sulphuric acid. 

With a specimen of pyrocatechin make the follow- 
ing tests : 

1.) To a few c. c. of an aqueous solution add several 
drops of potassium hydrate solution; set aside and notice 
the change that takes place in the course of an hour. 
What is this change due to? Add some pyrocatechin to 
a little urine and repeat the test. 

2.) To the dilute aqueous solution add some ferric 
chloride. Note the color produced— now add ammonium 
hydrate to alkaline reaction. What is the result? 
Acidify with acetic acid and the original color returns. 

3.) To about 1 c. c. of the aqueous solution add one 
drop of furfurol- water, then add slowly 1 c. c. of concen- 
trated sulphuric acid and in such a way that it runs 
down the side of the tube and collects at the bottom. 
The liquid becomes cherry-red in color, later violet. 



32 URINE ANALYSIS. 

4.) Examine the crystals and test the solubility in 
ether. 

5.) Warm with a little Fehling's solution. Observe 
the reduction. 

HYDROQUINONE', Ce H4 (0H)2 . 

Para-dioxybenzole (1.4). May appear in the urine 
after administration of benzole, phenol or hydroquinone, 
as an ether sulphuric acid. 

Test a little hydroquinone. 

1.) According to the directions given above under 
(1) and (5). 

2.) Rapidly heat a minute portion in a test-tube. 
Observe a violet vapor which condenses to an indigo-blue 
sublimate. 

How many different compounds are possible of having 
the formula 06H4(OH)2? Write their structural for- 
mulae. What is the meta-compound called? 

Compare the above compounds with uroleucinic and 
liomogentisinic acids (alkapton). 

AMIDO ACIDS. 

s s 

C YSTIN. (C3 He N SO2 )2 =CH3-C-NH3 NH2 -6-CH3 . 

CO2 H c'02 H 

Examine a specimen of the crystals under a micro- 
scope and sketch the form observed. 

Cystin can further be recognized 

1.) By its insolubility in water, alcohol or ether; 
soluble in mineral acids and alkalies. 

2.) In alkaline concentrated solution with benzoyl 
chloride (see p. 9) gives benzoyl cystin. 

3.) On boiling with potassium hydrate the sulphide 
of potassium forms and may be recognized by bringing it 
in contact with a bright silver coin. 

4.) Yields no murexide test (p. 16). 

How would you distinguish between uric acid, when 



THE URINE CONSTITUENTS. 33 

it occurs ill six-sided crj^stals in deposit in the urine, and 

cystin ? 

Cadaverine, O5 HuN2 = 

NH2 .CH2 .CH2 .CH2 .CH2 .CH., .mi, . 

Putrescin'e, C4 H^oN^ =NH2 .CH^ .CH2.GH2 .OH^ .NH^ . 

These ptomaines occur in the urine with cystin in 
cystinuria and can be isolated by the benzoyl chloride 
reaction (see p. 9). 

LEUCIN, Ce Ha3N02 . 

«— Amido caproic acid (isobutyl-acetic acid, Schulze and 
Likiernik). 
Leucin and tyrosin can be prepared by decomposing 
proteids (better white horn) with acids. Both have been 
prepared synthetically. 

Properties of leucin. 

1.) Examine a specimen of leucin under the micro- 
scope. Note the characteristic form. 

2.) Rather difficultly soluble in cold, more readily in 
warm water; easily in acids and alkalies. 

3.) On heating sublimes to a flocculent white mass 
and gives off an odor of amylamine. 

4.) Forms salts with acids and bases. The blue 
copper salt is very difficultly soluble. 

5.) Scherer's test. — Place some crystals on a platinum 
foil, add nitric acid and cautiously evaporate to dryness — 
a colorless scarcely visible residue remains. Now add 
a few drops of sodium hydrate and warm, when the 
residue dissolves forming a clear or slightly colored solu- 
tion. On cautious concentration an oily drop remains 
which does not moisten the foil but rolls about readily. 

Detection of leucin in the urine (see tyrosin p. 34). 

OH 

TYROSIN, CaHuNOs = 



OH3.CH(NH3).C03H. 
Para-oxyphenyl -a- amidopropionic acid. 



34 URINE ANALYSIS. 

When found in the urine, as in acute yellow atrophy 
of the liver, it is usually accompanied by leucin. May 
occur in sediment or in solution in the urine. 

Detection of leucin and tyrosin in urine.* 

Precipitate the urine with basic acetate of lead, filter 
and remove the lead from the filtrate by hydrogen sul- 
phide. Then concentrate the solution as low as possible 
and set aside to crystallize. Examine under the micro- 
scope for crystals of leucin and tyrosin. If leucin is 
present it can be removed by means of alcohol. 

Properties of tyrosin. 

1.) Crystallizes in bunches of delicate needles. Ex- 
amine a specimen under the microscope. 

2.) Very difficultly soluble in water and in alcohol ; 
readily in acids and alkalies. 

3.) To a warm aqueous solution of tyrosin add 
Millon's reagent. The solution becomes dark red, and a 
red precipitate forms. (Hoffmann's reaction). 

4.) Warm some tyrosin with a few drops of concen- 
trated sulphuric acid, then add water and barium carbon- 
ate to remove free acid, filter and to the neutral filtrate 
add a drop of neutral ferric chloride — violet color. 
(Piria's reaction). 

5.) Place some crystals of tyrosin on a platinum foil, 
add nitric acid (1.2 sp. gravity) and warm. The tyrosin 
becomes bright orange yellow and dissolves. The residue 
on evaporation, is strongly yellow colored and transparent. 
On contact with a drop of sodium hydrate a deep reddish- 
yellow solution results which when evaporate*! leaves an 
intense blackish-brown residue. (Scherer). 

PHOSPHORIC ACID, H3 PO4 . 

Exists chiefly in the urine as metallic salts— a minute 
amount exists as an ether phosphoric acid (glycerine-phos- 
phoric acid). 



THE URINE CONSTITUENTS. 35 

Phosphoric acid (HgPOijforms three series of salts: 
Normal— M3PO, 
• Monohydric— M3HPO, 
Dihydric- MH2PO, . 
What is meant by alkaline phosphates ? By earthy 
phosphates ? 

NEUTEAL CALCIUM PHOSPHATE, Ca3 (PO,),. 

1.) Heat some urine in a test-tube. Observe that it 
becomes cloudy ; add a drop of nitric acid and the cloudi- 
ness dissolves. What is it due to? 

2.) To some urine add sodium hydrate when a pre- 
cipitate of the phosphate of calcium and magnesium are 
thrown down. Examine the precipitate under the micro- 
scope. What is its appearance ? Test the solubility of the 
precipitate in acetic, hydrochloric and nitric acids. How 
would you distinguish between a deposit of amorphous 
phosphates and amorphous urates? Amorphous oxa- 
lates ? 

ACID PHOSPHATE OF CALCIUM, CaHPO^. 

To a solution of calcium chloride add some di-sodic 
hydric phosphate solution, drop by drop. Examine care- 
fully the characteristic form of the crystals. This salt is 
always cr3^stalline and is deposited in acid urine only. 

To some acid urine add dilute ammonium hydrate till 
only a faint acid reaction remains. Set aside till crystals 
form, then examine under the microscope. 

MAGNESIUM AMMONIUM PHOSPHATE, MgNH.PO,. 

Why is this salt spoken of as the triple phosphate ? 

1.) To some urine add ammonium hydrate and set 
aside over night — stellate or pennate crystals of triple 
XDhosphates form. Examine under the microscope. 

2.) Set some urine aside for. a few days. Ammoniacal 
fermentation sets in and the prismatic form of tnple 
phosphates is deposited. Examine the characteristic 
crystals. 



36 URINE ANALYSIS. 

This salt is not deposited in the urine unless ammonia 
is present. The reaction ma}^ be neutral or alkaline. If 
stellate crystals of triple phosphates are found in a urine 
what does it indicate? Are they of importance ? When 
Ijrismatic crystals of triple phosphates are found what does 
it snow ? When are they of importance ? 

How would you distinguish the short prismatic form 
of triple phosphates from crystals of oxalate of lime? 
What fact distinguishes triple phosphates from acid phos- 
phate of calcium ? 

ACETONE, CH3.CO.CH3. 

Detection in the Urine. 

To 250 c. c. of fresh urine (diabetic is best) add a few 
c. c. of acid and distil. Examine the first 10-20 c. c. of 
distillate by the following test: 

Lieben's Iodoform Test. 

To the acetone solution add some iodine in potassium 
iodide, then potassium hydrate till the iodine just clears 
oif — a yellowish-white cloud results. Allow to settle then 
examine for iodoform crystals — six-sided plates or stellate 
groups. 

To a few c. c. of water add some alcohol and test for. 
iodoform as just given. 

AOETACETIO ACID, C4 Hg O3 =CH3 .CO.CH^ .CO2 B. 

Detection. 

1.) To the urine (diabetic) add ferric chloride as 
long as a precipitate of phosphates form, filter and to the 
filtrate add some more ferric chloride — a wine-red color 
indicates acetacetic arid. 

2.) The urine on distillation yields acetone. 

CHOLESTERIN C26H43.OII . 

Tests of Recognition. 

1.) Crystallizes from alcohol in characteristic rhom- 
bic plates. Examine a specimen under the microscope. 



THE URINE CONSTITUENTS. 37 

2.) Insoluble in water, alkalies, dilute acids, cold 
alcohol ; readily soluble in hot alcohol, ether, chloroform. 

3.) To a few crystals on a slide under the microscope 
add a drop of concentrated sulphuric acid — the edges 
color a carmine-red. 

-t.) Dissolve a few crystals in a little chloroform, 
then add an equal volume of sulphuric acid, and shake ; 
the chloroform becomes blood-red, then cherry-red and 
purple. 

Detection in the Urine. 

Extract the urine with ether which takes up fat and 
cholesterin. Remove the ether layer and allow to evapor- 
ate spontaneously. Examine the residue under the micro- 
scope for the characteristic crystals of cholesterin. If 
there is any doubt, remove the fats by saponifying with 
potassium hydrate, dissolve in water, extract the solution 
with ether and proceed as above. 

FATS. 

Examine a drop of milk under the microscope and 
study the characteristics of the fatty globule. 

Fatty crystals can be recognized by melting when 
gentl}' warmed; solubility in ether. 

CLASSIFICATION OF PROTEIDS. 

(after Hammarsten). 

I. — Proteins, contain C,H,N,0,S; some contain P. 

Albumins=serum albumin, egg albumin, lactal- 
bumin. 

Globulins=serum globulin, fibrinogen, myosin, mus- 
culin. 

Nucleoalbumins=casein, (in bile, urine). ' 

Albuminates=acid albuminate, alkali albuminate. 

Albumoses, peptones. 

Coagulated proteins, as fibrin ; coagulated egg albu- 
min (by heat). 



38 UEINE ANALYSIS. 

ll.—Pfoteids. 

Mucins=real mucin, mucoids. 

Nucleins. 

Haemoglobin. 

Hyalogen. 
TIL — Alhu7ninoids 

Keratin. 

Elastin. 

Collagen. 

(Amyloid). 

General Reactions of Proteids. 

1.) Coagulation by heat. Albumin coagulates in a 
slightly acid or neutral solution ; haemoglobin and globulin 
require presence of a neutral salt ; nucleoalbumin requires 
acetic acid and thealbumoses need some sodium chloride. 
Peptones do not coagulate. 

2.) Mineral acids (as nitric) coagulate albumin and 
globulin. 

3.) Saturation of the solution with powdered ammo- 
nium sulphate precipitates all protems except peptones. 

4.) Salts of the heav}^ melals (as mercuric chloride, 
lead acetate, etc), precipitate most of the proteids. 

5.) Alcohol precipitates all proteids. 

6.) Phosphotungstic, phosphomolybdic, tannic and 
picric acid ; potassium ferrocyanide and acetic acid, mer- 
curic chloride, potassium mercuric iodide, etc., precipitate 
the proteids. (Alkaloidal reactions.) 

Color Reactions of Proteids. 

1.) Millon's Reaction. — To some albumin solution 
add Millon's reagent and warm slightly but not overheat. 
A precipitate forms which becomes colored red and the 
liquid likewise. This reaction is due to the aromatic nuc- 
leus in albumin ; is given by phenol, tyrosin, etc. 

2.) Xanthoproteic Eeaction. — Heat some albumin 
solution to boiling with strong nitric acid — yellow floccules 



THE URINE CONSTITUENTS. 39 

or a yellow solution results. Cool and add ammonium or 
sodium hydrate when the color changes to an orange- 
yellow. 

3.) Adamkieioicz's Reaction.— To a mixture of one 
volume of concentrated sulphuric acid and two volumes of 
glacial acetic acid add a little albumin (avoid too much) 
solution. The liquid turns, slowly on standing, more 
rapidly when slightly warmed, to a beautiful reddish 
violet. The reaction is not given by gelatin. 

4.) Biuret Test.— To an albumin solution add sodium 
or potassium hydrate, then a drop of very dilute copper 
sulphate. The solution becomes pink to violet according to 
the amount of copper sulphate used. 

5.) Liehermanii' s Reaction. — Heat some albumin with 
concentrated hydrochloric acid^a violet color is pro- 
duced. 

6.) Heat some albumin with concentrated sulphuric 
acid and a little sugar — a beautiful red color is the result. 

Under pathological conditions one or more of the fol- 
lowing proteids may appear in the urine : Serum albumin, 
serum globulin, albumoses, peptones, haemoglobin, methae- 
moglobin, fibrin and perhaps fibrinogen. 

ALBUMIN. 

Make the following tests with a solution of egg albu- 
min and then apply to an albuminous urine (filtered). 

1.) Coagulation Test. — Heat the specimen to boiling 
in a test tube ; whether a precipitate forms or not add 
some concentrated nitric acid. If a permanent cloudiness 
remains it indicates albumin; if it disappears it is due to 
phosphates. 

2.) Potassium Ferrocyanide and Acetic Acid Test. — 
Acidulate the specimen with acetic acid then add a few 
drops of potassium ferrocyanide when a precipitate forms. 
If the amount of the precipitate is small and its nature 
doubtful transfer it to a filter, wash and add ^ ^- c. of 
boiling Millon's reagent; or transfer a portion of the pre- 



40 URINE ANALYSIS. 

cipitale by means of a glass rod to a test tube and then 
add Millon's reagent— a reddish coloration indicates albu- 
min. (Winternitz). 

3.) Heller's Test. — Place some of the solution to be 
examined in a test-tube, and while holding it in an inclin- 
ed position pour in some strong nitric acid so that the acid 
does not mix but forms a separate layer at the bottom. 
If albumin is present a cloudy ring forms at the plane of 
contact. 

4.) Picric Acid Test.— To the solution add picric acid 
— a precipitate forms. 

5.) Acidulate the solution with acetic acid and add 
an equal volume of a saturated solution of common salt or 
magnesium sulphate and boil — a white precipitate forms. 

All these tests are given by globulin as well as albu- 
min. (For separate recognition see below). The tests 
commonly employed are those given under 1, 2 and 3, and 
are most delicate. 

GLOBULIN. 

This substance is present in most cases with albumin 
sometimes occurs alone. 

Detection of Globulin and Albumin in Urine. 

Neutralize 100 c.c. of urine and add powdered (120 g.) 
Mg S O4 , stirring well, till the solution is saturated. The 
globulin is precipitated. Filter and to the filtrate add an 
excess of acetic acid and boil. If a flocculent precipitate 
lorms it is albumin. (Hammarsten). 

ALBUMOSE. 

Detection in the Urine. 

Remove albumin, if any be present, by acidulating 
with acetic acid and heat. Apply the biuret test (p.) to 
the filtrate and if the result is positive then maki the 
Ibllowing tests : 

1.) To a portion add nitric acid— a precipitate forms, 
which on warming disappears and on cooling reappears. 



THE URINE CONSTITUENTS. 41 

2.) To another portion add acetic acid and potassium 
feiTocyanide — a precipitate forms which shows the same 
behavior. 

3.) Albumoses are precipitated by saturation with 

ammonium sulphate, or with sodium chloride in an acid 

solution. 

PEPTONES. 

Peptones are distinguislied from albumin, globulin 
and albumoses in not giving a precipitate with acetic acid 
and potassium ferrocyanide. From albumin and globu- 
lin in not precipitating on warming. Peptone is not pre- 
cipitated by ammonium sulphate. 

Detection of Peptones. 

To about 500 c. c. of the urine add just enough lead 
acetate to give a strong precipitate and filter. This 
removes mucin. Test the filtrate for albumin and if 
present remove in the following manner: Add a little 
sodium acetate and then concentrated ferric chloride till 
the mixture is blood-red in color. Then neutralize with 
potassium hydrate (or leave slightly acid), boil, cool and 
filter. The filtrate should give no precipitate with acetic 
acid and potassium ferroc3^anide (absence of iron and of 
albumin). If it is perfectly free make the following tests : 

1.) Add acetic acid and phosphotungstic acid — a 
cloudiness forms on standing if peptone is present. 

2.) If peptone is indicated by the above trial it can 
be isolated by the following method: Add 0. 1 volume of 
concentrated hydrochloric acid and then phosphotungstic 
acid also acidulated w4th hydrochloric acid, as long as a 
precipitate continues to form. Filter at once and wash 
with dilute sulphuric acid (3 to 5 c. c. in 100 c. c. water), 
till the filtrate is colorless. While the precipitate is still 
, moist mix with excess of powdered barium hydrate, add 
a little water, gently warm for a short time and filter. 
The filtrate contains the peptone ; apply the biuret test. 
(Hofmeister's method). 



42 URINE ANALYSIS. 

To Detect Kuhne's Peptone. 

Saturate the solution at the boiling point with ammo- 
nium sulphate and filter while boiling hot. Allow the 
filtrate to cool, decant the liquid from the crystals which 
separate, dilute strongly and predpitate the peptone by 
cautious addition of tannic acid. Let stand for 24 hours 
then filter. Boil the precipitate for a few minutes with 
baryta water filter and from the filtrate remove the excess 
ot barium by passing carbonic acid. Filter ofi" the barium 
carbonate and test the filtrate for biuret. 

HEMOGLOBIN. ' 

Thismay be found in the urine within blood corpuscles 
(Haematuria), or in simple solution (Haemoglobinuria). 

Detection of Haemoglobin in the Urine. 

1 ) Microscopic Examination. — Presence of blood cor- 
puscles and blood casts in the urine. 

2.) Spectroscopic Examination. — Place some blood 
in a test-tube (or better a shallow flask with parallel 
sides), and examine before the slit of a spectroscope. 
Notice the two black absorption bands and their position 
(oxy-haemoglobin). 

Now add some ammonium sulphide (or ammoniacal 
ferro tartrate solution) to the specimen and after awhile 
examine. Note the diff'erences in the spectrum since re- 
duced hgemoglobin has been formed. 

To the reduced haemoglobin solution now add a few 
drops of concentrated sodium hydrate and examine. 
Haemochromogen (reduced haematin) is formed. This 
test should be resorted to if the preceding are doubtful. 

To a specimen of blood add ferricyanide of potash and 
examine for the spectrum of methaBmoglobin. 

3.) Coagulation Test. — An aqueous haemoglobin solu- 
tion coagulates on heating. Albumin is always found 
if much blood is present. 



THE URINE CONSTITUENTS. 43 

4.) Heller'' s Test. — To the suspected urine add sodium- 
hydrate aud boil. The earthy phosphates are precipited 
and are colored red by the haematin. If there is any 
doubt filter off the precipitate and subject it to the hoemin 
test as follows : Place a portion on a slide, add a trace of 
common salt and a drop of glacial acetic acid and warm. 
Examine under the microscope for the characteristic 
rhombic plates of hsemin. 

5.) The urine may be precipitated with tannic acid 
and the precipitate examined by the haemin test as above. 

6.) Almeti's Guaiac Test. — Place in a test-tube equal 
volumes of a tincture of guaiac and old turpentine 
oil (containing ozone). The mixture mast not be blue. 
Now add the urine cautiously so that it forms a layer, 
when, if blood is present, a bluish-green ring will form at 
the zone of contact. 

Caution. — Pus may give the test with guaiac alone 

The urine if alkaline should be neutralized or rendered 

faintly acid. 

METHiEMOGLOBIN. 

This is recognized by the spectroscope, but care must 
be taken not to confound it with haematin. Distinguish by 
addition of ammonium sulphide (reduced haemoglobin 
forms) and by addition of ammonia. 

FIBRIN. 

Fibrin coagula are recognized by the insolubility in 
cold dilute acids or alkalies ; but soluble on prolonged 
warming. 

MUGIN-LIKE SUBSTANCE. 

To some normal urine in a conical test-glass add 
acetic acid. A delicate suspended cloud forms on standing. 
This is not real mucin but appears to be a nucleo-albumin. 

Properties. 

I.) It is precipitated by alcohol; b}^ acetic acid. 
2.) Dissolves in excess of mineral acids. In Heller's 
test nucleo-albumin, if present in excess, may react. 



44 URINE ANALYSIS. 

3.) Coagulates at 74 to 76°. 

4.) Gives the proteid alkaloidal and color reactions 
and is precipitated by the salts of heavy metals as mercury 
and lead. 

PUS. 

Examine a specimen of pus under the microscope and 
study the characteristics of the pus corpuscle. Apply a 
drop of acetic acid to the edge of the cover glass and note 
the effect. 

Detection in the Urine. 

1.) Pus Cells Under the Microscope^ — Recognized 
by the action of acetic acid and the mahogany brown 
stain with iodine in potassium iodide. 

2.) Donne's Test. — Decant the urine from the sedi- 
ment and add a piece of potassium hydrate and stir. The 
sediment is converted into a strongly slimy, sticky mass. 

3.) Test for albumin since it always accompanies 
pus. 

In strongly alkaline urine the pus cells soon disappear 
and the liquid becomes slimy. 

BILE. 

This secretion contains salts of taurocholic and glyco- 
coholic acids, and pigments as bilirubin and biliverdin. 

Pettenkofer's Test for Bile Acids. 

1.) To a dilute solution of bile in a test-tube, add about 
two-thirds its volume of concentrated sulphuric acid, 
slowly, so that the temperature does not rise over 60-70°, 
then add 2-3 drops of a sugar solution (1-10). The solu- 
tion becomes red, then violet. Avoid excess of sugar. 
The test depends upon the formation of furfurol. 

2.) Furfurol Test,— To 1 c. c. of the solution add 
one drop of a 0.1% aqueous furfurol solution. Then add 
slowly 1 c. c. of concentrated sulphuric acid and cool. 
Avoid excess of furfurol. 



THE URINE CONSTITUENTS. 45 

Detection in the Urine. 

This can be readily done if the urine is not too highly 
colored. If the latter is the case the acids must be isolated 
by Hoppe-Seyler's method. The urine is evaporated to a 
syrup and the residue extracted with strong alchohol. The 
alcoholic filtrate is evaporated to drive off the alcohol and 
the aqueous solution precipitated with lead acetate and 
ammonia. The precipitate is washed, treated with boil- 
ing alcohol and the solution filtered while hot. A few 
drops of soda solution are added to the filtrate and this 
then evaporated to dryness. The dry residue is extracted 
with absolute alcohol, the solution filtered, and to the 
filtrate ether is added in excess. On standing for some 
time the bile acids are precipitated and can be submitted 
to the test as above. 

Detection of Bile Pigments. 

l.)Gmelin^s Test. — Place some bile or the suspected 
urine in a small evaporating dish and add a drop or two 
of fuming nitric acid — a play of colors, green, blue to 
violet, results. 

With urine the green color is especially important 
since Indian may also give a blue color. Apply the same 
test with the following modifications : 

a.) To a few c. c. of fuming nitric acid in a test-tube 
add the urine cautiously so that the fluids do not mix — 
colors iorm at the plane of contact. 

b.) Filter the urine and then touch the moist filter 
paper with a drop of fuming nitric acid (Rosenbach). This 
is very delicate and especially valuable where the urine is 
highly colored. 

.2.) Hupperfs Reaction. — To the urine add a little 
calcium chloride, then an excess of ammonium hydrate — 
bilirubin-calcium compound is precipitated. Wash the 
precipitate on a filter, transfer while moist to a test-tube and 
fill it half full of alcohol which has been acidulated with 
sulphuric acid. Heat the mixture to boiling for some 
time— the solution becomes emerald to blaish-i^reen. 



46 URINE ANALYSIS. 

This test is especially applicable in very dark urines. 

3. To the urine add some tincture of iodine — an 
emeral -green color is produced. 

4.) Urate sediments can be examined by dissolving 
in sodium carbonate and then testing for bilirubin as 
above. 

GRAPE-8UGAR, C, R^ O, . 

Detection of Sugar in Urine. 

Make the following tests first with a sugar solution, 
then with diabetic urine. 

1.) Moor e- Heller'' s Test. — Render the urine strongly 
alkaline with sodium hydrate and boil. It becomes 
darker and earthy phosphates are precipitated. 

2.) Trommer^s Test. — Render the urine strongly 
alkaline as before then add a few drops of copper sulphate 
solution and warm — a red precipitate of cuprous oxide 
forms. 

2 a.) Feliling^s Test. — Boil some Fehling's solution in 
a test-tube and then add the suspected urine and boil- 
Cuprous oxide is thrown down. The urine if strongly acid 
should be rendered alkaline. This test is the one com- 
monly employed. 

3.) Bottger^s Test. — Render the specimen alkaline 
with sodium or potassium hydrate, then add a minute 
quantity of basic bismuth nitrate — a black color or pre- 
cipitate (bismuth ?) forms. Albumin if present must be 
removed. 

3 a.) Nylander^s Test. — Dissolve 10.33 g. sodium hy- 
drade in 100 c. c. of water; add 2 g. of basic bismuth 
nitrate, and 4 g. Rochelle salts ; warm and filter. This 
reagent keeps better than Fehling's solution. 

To 10 volumes of the urine add 1 volume of the 
reagent and boil 2-3 min. 

4.) Phenyl-hydrazine 7^e<§^5.-Phenyl hydrazine on heat- 
ing with sugar forms phenyl-glycosazone, Ce Hio O4 (N2 H. 
Ce Hg )2 . This forms bundles of yellow needles which 
melt at 204-205°. 



THE URINE CONSTITUENTS. 47 

Ce H,, Oe + 2 Ce H5 . N^ H3 = Cis ^22 N4 O4 + 2 H^ + 2 H. 

Application to the Urine. — Place in a small beaker 
about 50 c. c. of the urine add 1-2 g. of phenylhydra- 
zine hydrochloride and about 2-4 g. of sodium acetate, 
cover with a water glass and warm on the water-bath for 
about half an hour, then turn off the light and allow it to 
cool on the water bath. Examine under the microscope 
the deposit which forms. If amorphous dissolve on the 
filter in hot alcohol. To the filtrate add w^ater and boil till 
the alcohol is expelled— on cooling the characteristic yel- 
low crystals appear. 

5.) Fermentation Test. — Rub up some of the sus- 
pected urine with a little yeast. Fill the mixture into a 
large, wide test tube provided with a perforated stopper 
through which passes a tube bent into a U shape— the 
free arm being longer than the one that passes through 
the cork. Care should be taken to likewise fill the tube 
so that no air is present in the test-tube when it is in- 
verted. Set the tube aside m an inverted position in a 
warm place for 24 hours and observe the accumulation of 
gas. 

When the fermentation is completed place the tube in 
an upright position in a dish of water, remove the stopper 
and by means of a bent pipette introduce a little potas- 
sium hydrate solution. What is the result? 

CeHiA =2C-2H50H4- 2 0-2. 



PART II 



Quantitative Analysis of Urine. 



Quantitative analysis can' be carried out in two ways: 
gravimetrically or by weight, and volumetrically or by 
measure. 

In volumetric analj^sis the reagent is in solution in 
definite strength, and such solutions are spoken of as 
standard solutions. Standard solutions are of two kinds: 
empirical and normal. 

An empirical solution is one in which each c. c. indi- 
cates so much of the substance to be analyzed as may be 
desired. Thus, the solution of mercuric nitrate for the esti- 
mation of urea is made so that 1 c. c. of it represents 10 mg. 
of urea. Again, each c. c. of Fehling's solution represents 
5 mg. of sugar, and so on. 

A normal solution is one that contains in one litre 
one gram of basic hydrogen or its equivalent. Thus, a 
normal solution of hydrochloric acid (N HClj contains 
36.5 g. of HCl in one litre, since 1+ 35.5 (H + C1)=36.5. 
Again, H2SO,=2+32+64=98. But as 98 g. H^SO, con- 
tain 2 g. of H only one-half that amount is taken, i. e. 49 g. 
and dissolved in one litre. 

Calculate how much oxalic acid (CgHgO^ + 2H2O) is 
contained in a normal solution. 

The calculation for a normal alkali solution as sodium 
hydrate is as follows ; 

NaOH-fHCl=NaCl-^H20. 
40 36.5 



50 URINE ANALYSIS. 

40g. of sodium hydrate then combines with 36.5 g. of 
hydrochloric acid containing one gram of basic hydrogen. 
Therefore 40 g. NaOH in one litre make a normal solution. 

Calculate how much sodium carbonate (NagCOg) is 
contained in a normal solution. 

The normal solutions are too strong for most purposes 
and hence solutions of fractional strength are employed. 
Thus a semi-normal solution of hydrochloric acid is repre- 
sented by ^jgHCl which means that one litre contains one- 
half the normal amount i. e. 18.25 g. HCl. A decinormal 
solution (^lio) contains one-tenth the amount and a centi- 
normal solution (^|ioo) contains one-hundredth the amount 
that a normal one does. 

The word factor refers to the amount of the reagent 
contained in 1 c. c. of the solution. Thus, the N factor of 
NaOH is 0.040; the ^|io factor of hydrochloric acid is 
0.00365. 

The term titration is employed to denote the method 
of estimating a given substance in solution by means of a 
standard or titrated solution. Thus we can estimate chlo- 
rides in the urine by titration with an ^ho solution of 
silver nitrate. 

I. Determination of the Quantity of Urine per 

24 Hours. 

a.) hy volume — cylinders graduated in c. c. should be 
employed. 

b.) hy weight — more accurate but is less commonl}^ 
used. 

The average quantity of urine per 24 hours is placed 
at 1500 c. c. 

II. Determination of the Specific Gravity. 

a.) with the urinometer — The spindle of this instru- 
ment is graduated from l,000to 1,040 at a temperature of 
15° C. Hence, if the temperature is higher as is usuallj^ 
the case the observed reading should be reduced to the 
normal temperature of 15°. 



THE URINE CONSTITUENTS. 51 

Pour the urine to be tested into a cylinder which 
should be wide enou^'h to allow the urinometer free mo- 
tion. Avoid the formation of foam and if any results re- 
move it by means of a piece of filter paper. Immerse the 
clean dry urinometer and after it comes to rest read off 
the point where the lower border of the meniscus cuts the 
scale. To make sure that the instrument floats free gently 
touch tlie stem of the urinometer and after it comes to rest 
take a second reading. The normal specific gravity varies 
from 1017-1020. 

To reduce the observed reading to the normal tem- 
perature, take the temperature of the urine and for every 
3° above 15° add one division, and for every 3° below sub- 
tract one division from the observed reading. Thus, — 

The specific gravity of a urine is 1017 and the tem- 
perature 21°. 21—15=9. Therefore, 1017-f 3=1020, the 
correct reading. 

Reduction of the observed specific gravity to that cor- 
responding to the normal volume, 1500 c.c. Multiply the 
quantity of urine per 21 hours by the last two figures of 
the urinometer, divide by 1500 and add the result to 1000. 
Thus, the volume of a urine is 1820 c. c, the specific grav- 
ity 1011. 

1000+1^^^^=1017. 
1500 

Again, — The volume is 1500 c. c. the specific gravity 
1030. Therefore, 

1000 + ^^^^^^^=1090. 
1500 

6.) loith the picnometer or specific gravity bottle. 
This is the most accurate means for ascertaining the spe- 
cific gravity but is employed only for very exact work. 

III. Determination of Total Solids. 

a.) Neubauer's Approximate Method. — Multiply the 
last two figures of the urinometer by 2.33 which gives the 
weight of solids in 1000 c. c. To obtain the solids in the 

7 



52 URINE ANALYSIS. 

total 24 hours' urine multiply this result by the number 
of litres of urine. 

Examples: — The volume of urine is 1820 c. c. and the 
specific gravity lOM. 14x2.33x1.820=59.37 g. solids in 
24 hours' urine. 

The volume is 4500 c. c. and the specific gravity 1030 
30x2.33x4.500=314.55 g. solids per 24 hours urine. 

b.) Direct determination. — This is rarely resorted to 
except for scientific purposes. Inasmuch as a part of the 
urea is decomposed into ammonia and carbonic acid, the 
amount of ammonia given off must be determined, the re- 
sult converted into urea and the amount added to the 
weight of the residue obtained by evaporating on the 
water-bath a known quantity of urine. 

IV. Determination of the Acidity (or Alkalinity) 
of the Urine. 

Reagents. — . 

^lioNaOH solution. This contains 4g.NaOH in one litre : 
therefore each c. c.=0.004 g.NaOH, 

^!io Oxalic acid solution. This contains 6.3g. oxalic 
acid (H2C2O4+2H2O) in one litre, each c. c. =0.0063 g. 
oxalic acid. 

Preliminary exercise in titration. — Place 10 c. c. of the 
oxalic acid solution in a small beaker, add a drop of 
phenol-phthalein solution to serve as indicator, and then 
add from a burette, drop by drop, stirring after each addi- 
tion with a glass rod, the sodium hydrate solution until a 
permanent pink color remains. The difference in the 
reading of the burette before and at the close of the titra- 
tion gives the amount of sodium hydrate solution em- 
ployed to neutralize 10 c. c. of the ^|io oxalic acid. It 
should be 10 c. c. Why ? 

The readings of a burette should always be made with 
the eye on a level with the bottom of the meniscus. 

Application to the urine. — Owing to the color of the 
urine phenol-phthalein cannot unfortunately be used and 



THE URINE CONSTITUENTS. 53 

in its stead the less sensitive litmus paper is employed- 
Mix well the 24 hours urine and if any urates are present 
dissolve them by the aid of gentle heat, measure out 100 
c. c. into a beaker and from a burette run in ^ |io NaOH, drop 
by drop, stirring after each addition. Between each ad- 
dition the urine should be tested with litmus papers and 
the end-reaction is reached when the solution is neutral. 
When this is reached note the amount of ^|ioNaOH used. 
Ascertain by calculation the amount necessary to neutral- 
ize the total 24 hours urine. 

Example. — Suppose 100 c. c. of the urine requires 
3.4 c. c. ^|io NaOH and the 24 hours urine amounts to 
1250 c. c. 

100 : 3.4 :: 1250 : x. x=42.5 c. c. ^jioNaOH. 

Results can be expressed in this way but it is better to 
convert the number of c.c. of ^]io NaOH into the correspond- 
ing amount of oxalic acid. Each c. c. ^Iio NaOH=0.0063 g. 
oxalic acid. Therefore 42.5x0.0063=0.26775g. oxalic acid. 
That is to say, the acidity of the 24 hours urine corresponds 
to that much of oxalic acid. 

If the urine is alkaline the degrees of alkalinity can 
be ascertained by titrating with the ^|io oxalic acid. The 
result is converted into the corresponding amount of sod- 
ium hydrate. The results obtained by this method are not 
very exact. 

V. Determination of Chlorides. 

a.) Yolhard's Method. 

Reagents. — 

1.) Silver nitrate solution. — Dissolve 29.075 g. of fused 
silver nitrate in one litre of water. Each c. c.=10 mg. so- 
dium chloride. 

2.) A cold saturated solution of ferric alum, or a b% 
solution of ferric sulphate. This solution must be free from 
chlorides. It is used as an indicator. 

3.) Potassium sulphocyanate solution. — Dissolve about 



54 URINE ANALYSIS. 

10 g. of the salt in a ^ litre of water and standardize 
the solution against the silver nitrate. This is done as fol- 
lows: To 10 c. c. of the silver nitrate in a beaker add 5 
c. c. of a ferric solution and then nitric acid drop by drop 
till the mixture is colorless. Now run in from a burette 
the sulphocyanate solution, stirring well after each addi- 
tion, till a permanent red color is obtained. Note the 
amount used. 10 c. c. of one should equal 10 c. c. of the 
other. If the sulphocyanide is too strong it must be di- 
luted so that the two solutions have the same strength. 

Example:— 450 c. c. of the sulphocyanate solution is 
left in the cylinder and 10 c. c. of the silver nitrate solution 
requires 8.2 c. c. of the former. 10—8.2=1.8. That is, to 
every 8.2 c. c. of the sulphocyanide 1.8 c. c. water must be 

added. 

Therefore, 8.2 : 10 : : 450 : x= 548.8. 

The 450 c. c. in the cylinder diluted to 548.8 c. c. gives 
the solution of the proper strength. 

Execution. — In a flask provided with a 100 c. c. mark 
place 10 c. c. of urine, 20-30 drops of dilute nitre acid 
( 1.185 sp. gravity) then 2 c. c. of the ferric solution and 10- 
15 drops of a permanganate of potash solution (lOX). By 
agitating a little the color turns to a yellow. Now run in 
from a burette the silver solution till the precipitate ceases 
to form. Note the amount used. Fill up to the 100 c. c. 
mark with water, mix and filter through a dry filter. To 
50 c. c. of the filtrate run in from a burette the sulphocya- 
nate solution stirring well, till a permanent red tinge re- 
sults. Note the amount of sulphocyanate used, multiply 
it by two and deduct this from the amount of silver nitrate 
used. The difference is the amount of silver nitrate solu- 
tion which combined with the chlorine. Now calculate 
the amount of NaOl per 24 hours' urine. 

Example : — The 24 hours' urine amounts to 1250 c. c, 
and 10 c. c. of it required 14 c. c. of silver solution. Since 
each c. c. of silver solution equals 10 mg. of NaCl, 14 c. c- 
equals 14x10=140 mg.=0.140g. NaCl. 



THE URINE CONSTITUENTS. 55 

Now 10 : 0.140:: 1250 :x. x=17.59. NaOl per 24 hours, 
b.) Mohr's Method. 

Reagents. — 

1.) Silver nitrate solution of same strength as that 
used in Volhard's method. 

2.) A saturated solution of yellow potassium chro- 
mate (K2Cr O4 ). This must be free from chlorine and 
serves as an indicator. 

Execution. — Place 10 c. c. of the neutral or slightly 
acid urine in an evaporating dish, add about 100 c. c. of 
water and 2-3 drops of the potassium chromate solution. 
Now add from a burette the silver nitrate solution until a 
faint red tinge appears. This is due to the formation of sil- 
ver chromate and shows that all the chlorine has been pre- 
cipitated and an excess of silver added. Note the amount 
of silver solution used, deduct 1 c. c. and multiply the dif- 
ference by 10= mg. of sodium chloride in 10 c. c . of urine. 
Calculate the amount present in the 24 hours' urine. 

This method is more convenient than the preceding 
but give higher results. For that reason 0.5—1 c. c, is 
deducted from the observed reading. Albumin if present 
should be removed. When the urine is very dark it may 
be decolored by shaking with animal charcoal which how- 
ever must be free from chlorine. 

VI. Determination of Total Sulphuric acid. 

a) Gravimetrically. — Acidify a known quantity of 
urine with hydrochloric acid, add barium chloride and 
boil. Set aside for 6-8 hours., filter, wash with hot water, 
dry, ignite, and weigh. Deducting the weight of the 
ash gives the weight of the Ba SO4 . Calculate the 
amount of SO3 in the 24 hours' urine. 

b.) Yolumetvically . Reagent. — 
Dissolve 30.5 g of barium chloride (BaCl2 + 2 H2 O) in one 
litre. Each c. c. =10 mg. SO3 . 

Execution.— ^0 50-100 c. c. of the urine add 5-10 c. c. 
hydrochloric acid and boil for \ hour. Then from a burette 



56 URINE ANALYSIS. 

run in the barium chloride solution 1 c. c. at a time, as 
long as a distinct precipitate continues to form, mix and 
allow the precipitate to subside after each addition; when 
the formation of a precipitate becomes indistinct, to ascer- 
tain the point of neutralization, filter off after each addi- 
tion a few c. c. of the liquid and test for sulphuric acid by 
adding some barium chloride solution. If a precipitate 
forms pour it back into the beaker, add more barium 
chloride, mix and again filter off a small portion. Repeat 
this addition of reagent and testing until a filtered portion 
ceases to give a precipitate with barium chloride. Note 
the amounts employed the last two times. 

Thus suppose 17 c. c. barium chloride does not precipi- 
tate all the sulphuric acid whilst 18 c. c. does. Now take 
the same amo nnt of urine, treat as before, then run in the 
full amount of barium chloride solution up to next to 
the last addition — that is 17 c. c. Mix and test a little of 
the filtered solution, now add the reagent in smaller 
amounts than before, — about 0.2 c. c. at a time, testing 
after each addition, till the neutral point is reached. 

Note the amount of barium chloride used. Since each 
c. c.=10 mg. SO3 , calculate the amount of acid present 
in 24 hours' urine. 

VII. Determination of Phosphoric Acid. 

Reagents.— 

1.) Uranium acetate solution. — Dissolve 35 g. crystal- 
lized uranium acetate in a litre of water. This solution 
must be standardized against a standard solution of sodium 
phosphate so that each c. c. = 5 mg. P2 O5 . 

For this purpose dissolve 10.0845 g. crystallized Na2 
HPO4 +12 H2O in 1 litre of water, each c. c. =2 mg. 
P2 O5. 50 c. c.=0.1 g. P2O5 . 20 cc. of the uranium 
acetate solution should equal 50 c. c of this phosphate solu- 
tion. If not, calculate and make the necessary dilution as 
on p. 54. The titration is done according to the directions 
given below. 



THE URINE CONSTITUENTS. 57 

2.) d% acetic acid solution. — If uranium nitrate is used 
this solution must contain in addition 10% of sodium 
acetate in order to combine the nitric acid which would be 
set free in the reaction. 

3.) Tincture of cochineal, or solution of potassium fer- 
rocyanide as indicator. 

Ejcecution. — Place 50 c. c. in a beaker, add 5 c. c. of the 
acetic acid solution, a few drops of the cochineal tincture, 
and heat to boiling. Now run in from a burette the ura- 
nium acetate solution, stirring well, till the liquid becomes 
faintly or distinctly green and remains so when heated 
again to boiling the point. 

Note the number of c. c. employed, each c. c. =5 mg. 
P2 O3 . Calculate the amount present in the 24 hours 
urine. 

Potassium ferrocyanide solution can be used as an 
indicator instead of cochineal. For this purpose place a 
series of drops of the solution on a porcelain surface, or on 
a filter paper, and after each addition of uranium acetate 
to the urine, remove a drop from the beaker, by means of 
a glass rod and touch the ferrocyanide, a reddish brown 
color indicates the end-reaction, — that uranium acetate 
has been added in excess. 

VIII. Determination of Grape Sugar. 

1.) By titration with Feeling's solution. 

Reagent. — Dissolve 34.64 g. of crystallized copper sul- 
phate in ^ litre of water. Likewise dissolve 173 g. of 
Rochelle salts (potassium sodium tartrate) in about 200 c. c. 
of water, and 60 g. of sodium hydrate in 200 c. c. of water. 
Combine the two solutions and make up to ^ litre, then 
combine this with the copper solution and make up to 1 
litre. 

10 c. c. Fehling's solution=50 mg. sugar. 

Execution. — Run 10 c. c. of Fehling's solution from a 
burette into a 200 c. c. Erlenmeyer flask (or porcelain 
evaporating dish), add about 40 c. c. of water and heat to 



58 URINE ANALYSIS. 

boiling, now run in from a second burette the diluted 
urine 2 c. c. at a time till the blue color has disappeared 
and a yellow color remains. This can best be seen by 
holding up the flask in an inclined position before a win- 
dow. Allow the precipitate to partly subside after each 
addition, the better to see the color. When decoloration 
takes place note the amount of diluted urine used. 

Now repeat the titration with a new quantity of Feh- 
ling's solution, running into it at once the full amount of 
urine up to the point where copper was still seen last, after 
that add the urine in 0.5 c. c. quantity at a time till the 
copper disappears, note the amount required and calcu- 
late the amount of sugar in 24 hours' urine. 

Example : 

The quantity of urine for 24 hours is 4500 c. c. 

50 c. c. were diluted to 250 c. c. 

10 c. c. Fehling's solution required 10 c. c. of the 
diluted urine. 

Hence 12 c. c. contains .050 g. sugar. 

How much will 250 c. c. contain ? 

.050 : 12 : : cc : 250. :^ = 1.040 g. sugar ; that is 50 c. c. of 
undiluted urine contain 1.040 g. sugar. 

50 : 1.040 :: 4500 : it;, a: = 93.6 g. sugar. 

If albumin is present this should be removed, since it 
interferes with the settling of the precipitate. This can 
best be done as follows : To 100 c. c. of the urine add 10- 
15 c.c. of saturated salt solution, acidulate distinctly with 
a few drops of acetic acid and boil a few minutes, cool, 
make up to 100 c. c and filter. 

Before titration the urine should be diluted so that it 
contains at most 0.5X sugar. Measure out 50 c, c. of the 
urine and dilute to 250 c. c. If much sugar is present, i. e. 
if the specific gravity is over .0130, dilute to 500 c. c. 
2.) By fermentation. 

a.) From the difference in specific gravity, before 
and after fermentation. Determine the specific gravity of 



THE URINE CONSTITUENTS. 59 

fresh nrine. Take 200 c. c. add about 1 ^YRm of yeast and 
set aside in a covered beaker for 24—1:8 hours at a temper- 
ature of about 25° 0. Then filter the urine and determine 
the specific gravity at the same temperature as before. 
The difference between the two, multiplied by 230 (Rob- 
erts' factor), gives the amount of sugar in grams in 100 c. c. 
Calculate the amount in 24 hours urine. 

The results by. this method are quite satisfactory ; 
especially, if the urinometer reads to four decimal points,* 
or the specific gravity is determined by the picnometer. 

b.) From the amount of carbonic acid formed. — 

Einhorn's saccharimeter and similarly devised instru- 
ments can be used. 

c.) From the amount of alcohol formed. 
3.) Polarization method. This gives reliable results, 
though a trifle low. The expense of the instrument is 
such as to preclude its general use. 

IX. Determination of Nitrogen. 

1.) Dumas' Method. — 5. c. c. of the urine or more are 
acidulated with sulphuric acid and evaporated to dryness in 
a copper boat. This is then filled with copper oxide and 
X)laced in a combustion tube and heated. The nitrogen 
present is set free and is collected in a suitable apparatus 
and measured. From this, the amount ol nitrogen in the 
total urine can be calculated. 

2.) Kjeldahl's Method.— This is simpler than the pre- 
ceding and gives equally as good results. 5-10 c. c. of 
the urine are placed in a suitable flask, about 10 c. c. of 
strong sulphuric acid and 0.4 g. mercuric oxide added, and 
the mixture is heated till it is colorless. All the nitrogen 
has become converted into ammonia, and it is only neces- 
sary to distil the ammonia and estimate it to arrive at the 
amount of nitrogen present. 

3.) Yarrentrapp- Will's Method. — This is a very good 
method but not as simple in execution as the preceding. 
The residue of about 5 c. c. of urine is mixed with soda- 



6*0 URINE ANALYSIS. 

lime and ignited. The nitrogen present is converted to 
ammonia and this is estimated by receiving it into^|io acid 
solution. 

4.) Liebig^s Method for titration of urea gives results 
v^hich correspond very closely to the total nitrogen 
present, rather than to urea itself. For its description see 
below. 

X. Determination of Urea. 

1.) Liebig's Method. This as stated before is more 
nearly an estimate of the total nitrogen. 

Reagents. — 

Mercuric nitrate solntion. — Dissolve 77.2 g. mercuric 
oxide (or 71.48 g. mercury) in nitric acid and evaporate 
to drive off excess of acid, then take up in water and 
dilute to one litre. Each c. c. should equal 10 mg. urea. 
The solution should be standardized against a 2%^ urea 
solution. 

2.) Baryta Mixture. — Combine one volume of cold satur- 
ated barium nitrate with two volumes of cold saturated 
barium hydrate. This is used to remove phosphoric acid. 
3.) Solution of sodium carbonate containing 53 g. of 
the salt in one litre of water. This serves to indicate the 
end reaction. 

Execution. — To 40 c. c. of the urine add 20 c. c. baryta 
mixture, mix well and filter through a dry filter. Place 
15 c. c. of the clear filtrate, which corresponds to 10 c. c. 
of the original urine, in a beaker and run in the mercuric 
nitrate solution from a burette 1 c. c. at a time, stirring 
well after each adddition and testing with sodium carbon 
ate. This is best done by placing a series of drops of 
sodium carbonate by means of a glass rod on a porcelain 
surface and after each addition of reagent touching a drop 
with a drop of the mixture in the beaker. Continue the 
addition of the mercury solution till a distinct yellow col- 
oration is produced by the sodium carbonate. 

Now repeat the titration with a new portion, running 



THE URINE CONSTITUENTS. 61 

in the full amount up to the point short of the yellow 
color and from this add 0.2 c. c. at a time till the end 
reaction appears. Note the number of c. c. required, each 
c. c.=10 mg. urea. Calculate the amount in the 24 hours' 
urine. 

If much albumin is present it should be removed by 
the aid of heat and acetic acid. 

The above is the method as ordinarily and most easily 
employed. More exact results can be obtained if the 
chlorides present, are removed by precipitation with just 
sufficient silver nitrate. Why is it desirable ? 

Again, in the above method as seen from the follow- 
ing equation, nitric acid is set free. 

2 C0(NH2 ), + 4 Hg(N03 ) ^ + 4 Ho 0= 

2 C0(]SfH2 )^ .Hg (NO3 )2 .3 HgO+6 HNO3 . 

This free acid tends to alter the composition of the 
precipitate and to dissolve it, hence the solution should be 
carefully neutralized. 

2.) HtJFNER's Method. — This depends upon the fact 
that urea is decomposed by an alkaline solution of sodium 
hypobromate into nitrogen, carbonic acid and water* 

Reagent. — Alkaline hypobromite solution. Dissolve 
100 g. of sodium hydrate in 250 c. c. of water and when 
cold add 25 c. c. bromine. Keep in a cool dark place. 

Execution, — Place one c. c. of the urine in the lower 
bulb of Hiifner's apparatus, then fill it full of water up to 
the farther end of the perforation in the stopper. Now 
close the stopper. Fill the remainder of the apparatus 
and the measuring tube with the reagent. Close the 
mouth of the tube with a finder and invert over the appa- 
ratus so that no air enters, and place it into position. When 
this is done open up the stop-cock when the reagent 
passes into the bulb where the urine is and sets nitrogen 
free. This collects above in the measuring tube. In about 
a half an hour the operation is completed and the volume 
of gas can be measured with proper precautions. 



62 URINE ANALYSIS. 

From the volume of nitrogen the weight of the urea 
can be calculated according: to the formula — 



(._ v(b-bO 



354.5x760 (1+0.003665 t) 
G = weight of urea i v = volume of gas ; h —• baromet- 
ric pressure; b' aqueous tension at t° ; t=temperature. 

3.) Other methods for determination of urea are based 
upon its decomposition into ammonia and carbonic acid, 
but for ordinary purposes they are not available. 

4.) The specific gravity affords an approximate idea of 
the amount of urea present, provided sugar and albumin 
are absent. 
Thus, a sp. gravity of 1010 indicates about 1.0 % urea. 

" " " '' 1020 '-' a little less than 2% urea. 
Above this point the variation is too great to be of 
any value. 

XI. Determination of Uric Acid. 

1.) Method of Heintz. — Place 200 c. c. of urine in a 
beaker, add 5 c. c. cone, hydrochloric acid, mix and set 
aside for 24-48 hours in the cold. Filter through a prev- 
iously dried and weighed filter, transfer the crystals to 
the filter, wash with water till the chlorides are removed, 
then dry at 100-110° and weigh. The difference in the 
two weighings = uric acid. But as uric acid is not 
wholly insoluble in water, some of it is in solution. There- 
fore, measure the filtrate and wash-water and for ever3^ 
100 c. c. add 0.0048 g. to the amount of uric acid as found 
above. Now calculate the total amount in 24 hours' urine. 
By making this correction the method is as accurate as 
the following one. If urates are present they should be 
brought into solution by the aid of heat or addition of 
sodium hydrate. Albumin must be removed. 

Filter paper should not be weighed in the open air 
but should be placed in a weighing bottle or well corked 
test-tube. 



THE URINE CONSTITUENTS. 63 

2.) Method of Ludwig. 

Reagents.—!.') Ammoniacal silver nitrate sol u( ion. — 
Dissolve 26 g. of silver nitrate in water, add ammonium 
hydrate till the precipitate which first forms redissolves, 
then dilute to one litre. 

2.) Magnesia mixture. — Dissolve 100 g. of magnesium 
chloride in w^ater, add ammonium hydrate to strong excess 
arid then ammonium chloride till the precipitate is redis- 
solved. Dilute to one litre. The solution should be 
strongly ammoniacal. 

3.) Sodium or potassium sulphide solution. — Take 
15 g. of potassium hydrate (or 10 g. sodium hydrate), free 
from nitrous and nitric acids, and dissolve in one litre of 
water. Saturate one-half the solution with hydrogen sul- 
phide which forms KHS. Then combine the two solutions 
which gives K2 S. 

Execution. — To 100 c. c. of urine add a mixture of 10 
c. c. silver solution and 10 c. c. magnesia mixture and 
mix. If silver chloride is thrown down more ammonia 
is to be added ; if magnesium hydrate precipitates more 
ammonium chloride is needed. Allow the precipitate to 
settle, filter and wash 2-3 times with water to which a 
little ammonia has been added. Transfer all the precipi- 
tate to the filter. When the liquid has drained, transfer 
by means of a glass rod the moist precipitate to a beaker, 
place the beaker under the funnel and wash the residue 
on the filter with a boiling mixture of 10 c. c. potassium 
sulphide solution and 10 c. c. water. Heat on a water-bath 
for some time andwhen the entire precipitate is black filter 
through the filter previously used. Collect the filtrate in 
a dish and wash the filter with hot water. To the com- 
bined filtrate and wash-water add 5 c. c. of dilute hydro- 
chloric acid and concentrate to 10-15 c. c. Set aside to 
cool and in about a half an hour all the uric acid will have 
crystallized out. Filter through a glass, wool or paper 
filter, (Ludwig's filter) previously dried at 110° and weigh- 
ed. Wash with little w^ater, then dry and wash three 



64 URINE ANALYSIS. . ^ 

times with carbon bisulphide to remove sulphur, then 
with ether. Finally dry at 110° and weigh. The differ- 
ence in the two weighings gives the amount of uric acid. 
Calculate the amount present in 24 hours' urine. 

If albumin is present it should be removed according 
to the method on p. 58. 

3.) Hay craft'' s Method, — This is a volumetric method 
based upon the preceding and gives somewhat higher 
results. The uric acid is thrown out of solution and the 
precipitate washed as above. Then it is dissolved in nitric 
acid and the dissolved silver titrated with an ^Iso potassium 
sulphocyanate solution (see p. 51). Each c. c. used=3.36 
mg. uric acid. 

4.) Czapelts Method. — This method is the comple- 
ment of Haycraft's. That is, instead of estimating the 
silver in the precipitate, the silver in the filtrate is deter- 
mined and the difference betv/een this amount and the 
total amount added gives the amount of silver that com- 
bined with uric acid. The results are likewise higher than 
by Ludwig's method. 

XII. Determination of Albumin (and Globulin). 

1.) iScherer^s Method. — Place 100 c. c. of the clear urine 
in a small beaker. If much albumin is present, take less 
and dilute. If the reaction is not distinctly acid add a 
minute drop of acetic acid and heat on the water-bath for 
about i hour. The beaker should be covered and so 
placed that the lower half containing the urine passes 
through the ring of the water- bath. Heat till a coagulum 
of course floccules forms. The addition of a minute 
amount of acid aids this, but a larger amount must be 
avoided. Filter through a weighed filter, previously dried 
at 120-130°. Care being taken to transfer all the precipi- 
tate — a glass rod having one end covered with a piece of 
rubber tubing can be used to advantage. Wash with hot 
water till the precipitate ceases to give the chloride reac- 
tion. Then fill the funnel several times with absolute 



THE URINE CONSTITUENTS. 65 

alcohol, then twice with ether (to remove fats), dry at 
120-130° till the weight is constant. 

It is well to make always a few preliminary tests on 
the completeness of coagulation. For this purpose test 
the reaction and if acid, place some urine in a test-tube 
and heat in a water-bath till coagulated, then for a few 
minutes in the flame and filter. If the filtrate is cloudy 
or on testing with acetic acid and potassium ferrocj'-anide 
gives a cloudiness the urine is not sufficiently acid and a 
drop or so of acetic acid must be added. In this way 
make one or mere tests till complete precipitation is 
obtained and then acidulate to the proper degree the 
amount of urine taken for the estimation. 

2.) Densimetric Method, — In this method the specific 
gravity of the urine before and after coagulation is deter- 
mined and the difference in the specific gravities multiplied 
by 400 (Zahor's factor) gives grams of albumin in 100 c. c. 

The amount of acetic acid necessary to coagulate is 
ascertained as given above. This amount is then added 
to the urine and the specific gravity determined. The 
caguiation should be carried on so that no water is lost by 
evaporation and for that purpose, the urine is placed in a 
bottle provided with a rubber stopper and clamp (beer 
bottle). This is now immersed in water and heated to 
boiling for 10-15 min. The flask is then cooled, contents 
filtered and the specific gravity of the filtrate determined. 

The urinometers employed should read to four deci- 
mal points, or better still the specific gravity should be 
determined by means of a picnometer. The results are 
excellent and approach closely the gravimetric results. 

3.) Roberts- StolnikoiF Method. — A solution containing 
3^ mg. of albumin in 100 c. c. gives a faint but distinct 
reaction with Heller's test in 2-3 min. Hence dilute 
the urine under examination till it gives the test under 
these conditions. Then calculate the amount of albumin 
present in 24 hours urine. The results are sufficiently 
good clinically. 



6(j URINE ANALYSIS. 

4.) Eshach^s Alhumino meter. 

Reagent. — 10 g. of picric acid and 20 g. of citric acid 
are dissolved in one litre of water. 

Method, — The instrument is filled with urine to the U 
mark, then with the reagent to the mark R. The tube is 
closed with a stopper, inverted several times and then set 
aside in an upright position for 24 hours. Read off the 
height of the precipitate in the tube. The figures indicate 
grams of albumin in one litre. 

If much albumin is present the urine should first be 
diluted. The specific gravity should be 1010 or lower. 

The result obtained by this method are only roughly 
approximate but owing to simplicity of execution can be 
used for clinical purposes. 

XIII. Separate Determination of Globulin and 
Albumin. 

1.) Hammarsten's Method.— ^Qn&QY the urine slightly 
alkaline with potassium hydrate, filter if necessary to re- 
move phosphates. Measure out 25-100 c. c. according to 
the amount of albumin present and place in a beaker. 
For 100 c. c. add 120 g. of pulverized magnesium sulphate, 
stir well, and set aside for 21 hours in the cold. Filter 
through a weighed filter, previously dried at 110° ; rinse 
out the beaker with saturated magnesium sulphate solu- 
tion and wash with the same till the filtrate cease to give 
a reaction for albumin on heating with acetic acid. Then 
dry the filtrate at 110° (to coagulate the globulin) for 
several hours, cool and wash with hot water till all mag- 
nesium sulphate is removed. Then wash with alcohol 
and ether, dry at 110° till the weight is constant, cool 
and weigh. The difference = globulin -f some inorganic 
matter. Hence, ignite the filter and weigh the ash. 
Subtract the weight of the ash from the weight of the 
globulin as first found= weight of globulin. Calculate 
the amount in the 24 hours' urine. 



THE URINE CONSTITUENTS. 67 

If the total proteid is determined by Scherer's method, 
the difference between the two results gives albumin. 

2.) FohVs Method. --In this the urine is precipitated 
with an equal volume of a saturated solution of ammonium 
sulphate and the precipitate washed with a semi-saturated 
solution of the same. After that the process is the same 
as that given above. 

The results are about the same as those obtained by 
Hammarsten's method, and moreover the method possess- 
es the advantage that the (liter does not clog. 

XIV. Determination of Peptone (and albiimoses). 

1.) Method of Konig and Kisch.- — 50-100 c. c. of the 
urine (or a larger quantity) are concentrated to about 10 
c. c. The solution is precipitated by 100 c. c. of a satur- 
ated solution of ammonium sulphate in the cold, and 
filtered through a dried and weighed filter. The residue 
is washed with concentrated ammonium sulphate, then 
dried and weighed (B). The weighing bottle and filter 
are then washed with 500 c. c. of water and the sulphuric 
acid determined in 100 c. c, of the filtrate by precipitating 
with barium chloride and hydrocliloric acid. The weight 
of the BaSOi found x 0.536=- ( NH4 )-2 SO4 . This weight 
X 5= weight 01 (NH4 )2 SO4 held on the filter. Hence 
subtracting the weight of the filter and the weight of the 
(NH4 )2 SO4 from the weight of the precipitate (B) = 

weight of ALBUMOSES. 

Another portion of 50-100 c. c. urine (or more) is 
strongly aciduhited with sulphuric acid, then treated with 
an acid solution of sodium phosphotungstate (1 volume 
dilute H2SO4+3 volumes of sodium phosphotungstate 
solution) as long as a precipitate forms. The precipitate 
is filtered and washed with dilute sulphuric acid (1 : 3) ; 
the filter witli contents placed in a flask and the nitrogen 
determined by Kjeldahl's method. The weight of nitrogen 
X 6.25= weight of ALBUMOSES and peptones. (The factor 
for peptone alone is 6.41). 



68 URINE ANALYSIS. 

The weight of albumoses as found above subtracted 
from this gives the weight of peptone. 

If albumin and globulin are present they must be re- 
moved. 

2.) Maixner^s ColorimetriG Method— The peptone is 
precipitated and isolated according to Hofmeister's 
method as given on p. 41. With the solution of peptone 
thus obtained the biuret test is made and the color pro- 
duced is compared with that obtained from a solution of 
peptone of known strength. 



THE URINE CONSTITUENTS. 69 

AVERAGE C03IP0SITI0N OF URINE (AFTER SCHOTTEN). 

Average quantiry per 2^1: hours is placed at about 
1500 c. c. 

I. Normal Constituents. — 60 g. 
A. — Organic, — 35 g. 

Urea, 30 g. , 

Uric acid, 0.6 g. 

Creatinine, 0.8 g. 
, Xanthine compounds, oxalic acid, oxaluric acid, 
volatile fatty acids, lactic acid, glycerine-phos- 
phoric acid, suiphocyanic acid. 

Hippuric acid, phenol, cresol, pyrocatechin,indoxyl- 
skatoxyl sulphuric acids, oxyphenylacetic acid, 
hydrocumaric acid. 

Urine pigments. 

Ferments, sulphur and nitrogen containing sub- 
stances; substances of unknown composition free 
from sulphur and nitrogen. Total a few grams. 
B. — Inorganic, — 25 g. 

Common salt, 15 g. 

Sulphuric acid, 2.5 g. 

Phosphoric anhydride, 2.5 g. 

Nitric acid, 0.1 g. (or less) 

Potassium oxide, 3.0 g. 

Ammonia, 0.7 g. 

Magnesium oxide, 0.5 g. 

Calcium oxide, 0.3 g. 

Iron, 0.01 g. (or less) 

II. Ahnormal Pathological Constituents. 
Albumin, -^-oxybutyric acid. 
Globulin, Blood, blood pigments, 
Albumose, Melanine and other pigments, 
Peptone, Bile, pigments and acids. 
Mucin, Fat, cholesterin, lecithin, 
Grape sugar, Leucin, tyrosin. 
Milk-sugar, Alkapton (uroleucinic and 
Levulose, homogentisinic acids). 
Inosite, Cystin, putrescine, cadaverine, 
Acetone, acetacetic acid, Hydrogen sulphide, 



70 



URINE ANALYSIS. 



ANALYSIS OF 24 HOUES URINE. 



Volume, c. c — 
Specific gravity. 



Total solids. 
Water 



Organic substances- - 
Inorganic substances- 



Total nitrogen 

Urea 

Uric acid 

Creatinine 

Ammonia 

Hippuric acid ■ 

Phenol 

Potassium oxide 

Sodium oxide 

Sodium chloride 

Calcium oxide 

Magnesium oxide 

Chlorine 

Phosphoric anhydride (P2 O5 )--- 

Sulphuric anhydride (SO3 ) 

Sulphuric acid from sulphur con- 
taining organic substances 



Man. 



Meat. 



1672 



67.2 
1.398 
2.163 



3.308 
3.991 



0.328 
0.294 
3.817 
3.437 
4.674 



Bread, 



1920 



20.6 
0.253 
0.961 



1.314 
3.923 

0.339 
0.139 
4.996 
1.658 
1.265 



Horse. 



2055 
1.046 



248.244 
1806.755 

198.061 
50.183 

65.34 

traces 

0.357 

15.597 

2.445 



27.126 
5.713 



0.2199 
10.299 



3.165 



The results given in columns 1 and 2 were obtained by Bunge 
from the urine of the same individual under exclusive meat and 
vegetable diet, and each column represents the analysis of a single 
24 hours' urine. The analytical results in column 3 are those of E. 
Salkowski. 



PART III. 

EXAMINATION OF URINE SUSPECTED TO BE ABNORMAL.* 

Collect the urine for the twenty-four hours, mix and measure 
it. Ascertain the specific 2;raYity and reaction. Set a portion aside 
in a clean glass vessel (better, a conical one) and allow the deposit 
to subside for microscopical examination, as given in the following 
tables (A), (B) and (C). Filter another portion any test the clear 
filtrate according to table (D). 

MICROSCOPICAL EXAMINATION OF UEINARY DEPOSITS. 

Allow the urine to stand in a glass vessel undisturbed for some 
time ; then by means of a small pipette or dipping rod, take a drop 
from the bottom of the vessel ; place the drop on a glass slide ; 
cover with a thin glass and examine under a microscope which mag- 
nifies from 300 to 500 diameters. The objects seen under the micro- 
scope may be either crystallized, amorphous, or anatomical. The 
same substance may appear at one time in crystals, and at another 
in the amorphous form, and may thus indicate different pathologi- 
cal results ; consequently, the following tables are given : 

* We are greatly indebted to Professor V. C. Vaughan who has 
kindly authorized the reprint of the following directions and tables. 
They are taken from his Handbook of Chemical Physiology and 
Pathology, 3rd edition, p. 323. 



72 



URINE ANALYSIS. 



o 



?H C 0). 



02 p o 



'^ 9 a 



ce^ 



000 






o 
^2 ^-^ 



O 0) 



^ oi iS 



<X> f-t <^ 

^ p S 
d .d "^ 






o 



d^ 



o 



^ OS o 



CD d 

w ;i u . o c^ 

« i:; p i:^ c^ ^ 

OrG d Q)^ d 

'^ -^ p ^ &-0 

.S S S ^ d'-^ 



oa c^ 



o3 6J3 
^ P.>.d ^5 p 



t^-l a; d 
- -^ d d J g 



OP a^ 

d O c3^ 



H 5r3 d c3 o 

r-; CS O p O 

^ - cj ^ O 



I— I -ri ^ 

00 p 

^ ce - 

o P ^ 

■^ "^j ^. 

+^ ^ ^ 

O -4-^ -tJ 



(D 00 



d ^;t^ 

O 00 
c^ 00 00 



d^ p 

rc!-;qp 



OQ 



CO o) ^ 

CC » O 
O) '^ O 

+J -t-i rC 

+-I O) o 

^_a^ 

CD '^ -^ 

Si ^d 






Sh ce O) 

I— 3 c: ^ on 



a-' « 
=^ "-■ ^ 

o.d "d 

-^ a^. 

^S d 



CO f-; 
O d 

N d 

1.2 



O 0^ 



p ^ 

id CD 

d o 



d p ^ 

P o5 P 



o a 

03 






m 



cS 






-^ 


"Zs 





O) 


a 




^• 


d 


Q 


*'"' 



0^ b p 
dH=* '^'^ 

J 0= 3 ^ c 



32:5 o 
a o 






^2 



'^ o 



O) OS S ^-^ 
^, IS 5^3 2 ^ 

oi'P ppd o) 






•■dTd 

c^ho d 

..rt an""' 

d ord 




Ph 



^^d 
o a g 

dJ P -d 

a; 



ft fH 



P Oi 

3§ft 

(^ drd 

2 S ft 





CO d 

o.S 

rd O 



IHE URINE OONSTlTtESTS. 



73 






o g 
03 



- si 2 §1 I 

m 



c3 g; H 



ga 



5 0) 32 i>^ P^ 5 O 
«+=< s^ 9^ ce S *^ -43 



" ^ r- "-" ►^ 



^ ^ o 2 o'i^^ 2is 
p:2 bjj:^ 2i3 g::3 c5 

^ CD '^ CE JJ~ 5 

^ - J ^ i 



•i;^-^J|.2^^2 



©bog 



&>^>>^.S^j2i-^§ 



53 

c3 ce 



'^ rt ^ ;= s 






s-i !^ jh ^ .;^ 



c3 o o 

<^ ^ D <^ 2 2 fl 



a'v, o 









■-(-I ^ S o ^ 

Q o ^ ::; 



.91 

QQ 



X 



,005 



^ 3^ -^xt^ 2 p'C,2 =^'g 

;fla)><ic^-^0!-.^;p <-- 
E-i^ o p^ Cl, p^ ci, :z c o 



^ -^ "c^ 



ce w 



-M r^ P P I— ' 

p ."^ o ce ^ 

0^,2rP^ 

SQ -^J -1-3 -^J -tJ 



OC ^ QQ 




Pr-— ' 




2s'^ 




no 


73 o-^ 


^ 


O) rH r— 


t3 


3-- ^ 


'^ 














->' 







p ce 




Oir^ 




«le 




t^ 








Si 




^ 




ce 




?H ^ . 




^^ Q 




^ £= P 





.2ces^3^^^g 



CB.4:i-Ptfl 
ce >, 

p^ 



(D 



© ce 0^ o 
o « 

o -^ ce ;>, o) o --< 



O -^ 

O P O Ph 



P =^ 

^^ 

^p-3 CD 



O 

ce ^• 
le P 

X 

C p 



74 



VrW^ AMALYiI§. 



OQ O 



5 o s^ 

b '^ fl 
j; o) y 

0:30 






C3 



g c a «^ 



O) 



O) 



CC 



03 



EC o 



§§-s 

- S =! 
'^ d eg 



g-5 

SIP 

,30 a) eg ^ 



^ eg c ^ 
pq jH g o 

O &iD 

a 
';:::i 'TD T3 S 



G O ^ »^ 






ftp ?H 

CD ^^ eg © 

CC u a; (D 

00 c fi; <5 



-'-^ ?i- _ w 
c © s o 

eg * C o 

a^S,3 



'^.j 



•- p3 



■X) <D 



eg Oiki-ti 
a:) 






^ O) H 
O P eg: 



^" « r^ «Q 
fl 0) gT3 

O) O O '"^ 

eg fl eg^ 
o -^ 

•" OQ O 

G ^ O 

0) 0) O 

2 o Q 
^-^^ a> 

«g ?H.t;5 

lU O O/ H 




eg oc o 

P-d eg 

^ i~:j eg 
^ a O 

o ^ ' — ' 

>-H ^ CO 

Ph— eg 
eg 1i -t^ 
02 O O 



^ O^ 2 S © 
g •-:? O -Id '2 ^ 



_0 eg eg 



^^ 



c; eg --^ tit o 
C ,, CD _g C 

' a> rj (D OD^ -^ 

v::':^ J. o ^:; 

rH^^ CD t^ Og 

o .ti o ^ o 

r- ^^ 2 ^ 

a:^-^ <^'t^ ^V 

P^ eg ;:_ CD eg --< 

B ^;=: -M 2 

-. -^ -^ qqn ^ 



S3 



;^ c 



9^ ^ 



0) 



^^ 



p c 



4 ^ o eg O 



P CO CC 

S-l "^ 4^ 



ox;, ^ 0) 

(1) (D CD eg fp 
^^^ ><^ 

Fj ^^ CC O Siji 

o .22 -P o .^ 3 

^^0. O 0) - 



o o 



CD ;>,43 
=0 P eg 

O P 
^,P 2 

q; g CO 



P a O g;) p 

S P ^ &J0 eg 

p.r- a; a a: 

0^2 £i^ 

p ^ P t^ =3 

p ^ - ^ a 

S ^ S a =i 



11 



p & g 

o P 

^cg ?3 

.^^ a. 




P ^ 

^ o • 



P.3 

Jp o 



P I? 



|i 

eg -^ 



THE URINE CONSTITUENTS. 



75 



o 



CD ^3 ?? S 






a; a> aQ 



o fl 



O) 



O hS 

S S 0^ =! "^ 



5^-5 f^ 



g ^^ CD O^^.co O ^g-?:; 

•r-(^ CD^ ;^_ ^-(-^-►J >)^ A 



o ;^ 

'^ '^i 73 



:3 ao 






^.2 -Si 
51 gg 



^-^ .2 3 

^ •" o 1e '^ 

Hi — ( ^^T^ 

'^ 13 -a '3 52 T3 ^ ^ '-^ 2 
02^. X a; :=.^co :: o rt 
- -■ - ■ -■ ' ' o o 



- 2 CO <i> 

-5 32 f3 f-H 



g-;^J 



a; cj PhTS ce 4^ o 



^ r-; q:) 






~ o 



^ o 






P CO 

CO 5h 
_ O 



2 



•S ce 3 H 



g O C^ ^ 

^^.2-3 
'3 ^(^ ^ 



<1 



3 2 



2-2 



a; 
.2 

03 -(J 









O 



76 



URINE ANALYSIS. 



O 

< 

m 

CO 

o 



o 

'bii 

o 

1 


generation of the kidneys and in chy- 
luria. 

Crystals of calcium sulphate have 
been found spontaneously deposited in 
human urine. These crystals may be 
obtained from the urine of the horse. 

A deposit of hippuric acid indicates 
an excess of this constituent, and is gen- 
erally due to the kind of food. 


Chemical Tests. 


in globules resembling oil, 
when it should be collected 
and dissolved in boiling al- 
cohol, and allowed to crys- 
tallize. 

The needles of calcium 
sulphate dissolve on the ad- 
dition of an excess of water. 
They are distinguished from 
those of tyrosin by the in- 
solubility of the sulphate in 
ammonia. 

Easily dissolves on the ap- 
plication of heat. 


fa - - 


terestic notch 
in one corner. 

In fine needles 
resembling ty- 
rosin. 

In needles or 
rhombic 

prisms. 


Reaction of the 
urine in which 
the deposit oc- 
curs. 


Acid. 
Acid. 


6 

a 

es 


Calcium sul- 
phate. 

Hippuric acid. 



THE URINE CONSTITUENTS. 



77 



M 



9 I 




0) 


CO 

g 


T3 


o 


2 


o 

=2 


^ 

TS 

S 


CD 


o 


'^ 


ci 


"- 


a) 




rr 


rt 


>^ 


a 


g 






0) 


a 


so 


o 


g 
'o 




.22 










dJr^ 




^ 


O 


C3 


'02 

o 

r3 


^ 


'rt 


cS 


Qj 


H-3 

o 


§ 


CD 

a 

*5^ 


8 


'o 
? 




^ 
Oi 






o 


X 


s-T 


.9 










o 




a; 


rr 


^ 




;:; 


.^ 


02 a; 


a; 


£ 
rt 
o 


.i 1 


o 


• 1—1 


(S 


^ 


4-1 


I— 1 




<D 


r^ 


'S 


o 


o 





r-^'C! 



^ A't; 



o > 
^ o 

2 0) 



11 

CS CD 

CO O 

O (D 
Ores 



CO !h ^-1 









c5 cS 

o 



^ C3 

O :j 

O O) 

•^ be 

50 J2 

<x) a 



■<^ oo a^ 
'^ -a 

a a >= 



0^^ ■" 

.rt OD O K 
O'T^ 0) ci Oi 

'^ o'p.-rra 



i^ i^ ^ 

•S o ^ 

a:, 02 



'^isM^^ 



P>j.X r-i O CO 

%-! ^ a n q:> 



p" o ^ "^ a 

""^l^ 2 2 o 
u 5 o a c 



o) c; 



a; 



'^='_^|2?. 
a 



o 
S >^ 



3 i-^ cS K "^ ce ■ 

: ^ 2 'rt '^ K^^ . 



cD-:^ 

32 50 

•= a 






a a 

biO-T; 



0) 



'r. o^ 



fB a :i 
_<D ^ a 

;::^ CD -^ 
o 



p 

^ 'c5 "IJ 



arg O'^ S 

I— I ^ a o 
?^ a =4-1 si 



r-l Q) 

■c23 




ir 



a 

a . 
>^a 

5h c3 

5h ;=! 



c^a 
so a 

2-3 



1 Ph 



78 



URINE ANALYSIS. 



W 



m 
O 

i 

o 

"'3 

1 

s 

o 


Urates are the most common constitu- 
ents of urinary deposits. They vary in 
color from white to crimson : the higher 
the color the more serious the indica- 
tion. An occasional deposit of urates 
may appear from very trivial causes : as 
from a change in diet, in the amount of 
exercise taken and in the temperature. 
A deposit of urates occurring in acute 
inflammatory diseases is an indication 
for the better, showing that so much of 
the poison has been eliminated. But a 
constantly recurring deposit of urates is 
to be regarded as indicative of some dis- 
ease of the heart, liver, lungs or spleen. 


i 

1 

s 


to yield crystals of free uric acid on be- 
ing treated with acetic acid. 

Determine the presence of urates as in 
(A). It now remains to determine the 
base with which the uric acid is combin- 
ed ; collect the urates upon a filter ; place 
some of this collected deposit upon a 
piece of platinum and heat in the flame 
of a Bunsen burner or spirit lamp; (1) 
it communicates an intense yellow color 
to the flame, sodium urate; (2) it imparts 
a violet color to the flame, potassium 
urate. Remove another portion of the 
collected deposit to a clean porcelain 
dish, add a little potassium hydrate and 
then heat ; if the vapor of ammonia is 
given off, and colors a red litmus paper 
held over the dish, the deposit contains 
ammonium, urate. 


Reaction of the urine 
in which the deposit 
occurs. 


Acid, the urate of 
ammonium is not 
un frequently 
found in ammoni- 
acal urine. 


<i3 


02 



THE URINE CONSTITUENTS 



79 



Q 



C 
1 

o 
'So 

C3 


1 -4J 

S a; 

^ a 


ly contain much mucus, giving 
I ropy consistency, and the urine 
itly be alkaline from a volatile 


<S 
CD 

CJ 
CD 
> 

'4I3 

*— 1 


1 
CO 


CO 

'a! 


'^ 
CD 

+3 

Id 


<D 


.2 

'413 
h 

0) 


'S 


'^ 

m 

m 
<A 

CD 

1 


er part of the pus. 
nee of blood in the urine may be 
a physiological (as in menstru- 
a pathological haemorrhage. If 
ts large enough to be visible to 
eye, the blood must have passed 
le below the secreting structures, 
bladder the clots will often be 
and may obstruct the passage 
urethra. If the coagulation has 
in the ureters, the shape and 
lots will so indicate. AVhenfrom 
of the kidney, the coagula are 
er than those from the bladder, 
eserve the shape of the calices. 


(li 


CO 


— ( 

O 
42 


1 
> 


O 

03 




2 

'o 


-2 




CD 


"in 


2 si a 


O <^ ^ rC So'^ (^ so i; ft 

c3::3.as s^:s^"s^ a S 




















" 








F— C 1 


, , 


bx) 


§- 
























c; co.;^ 




1 


o 
























S8§ 
Z <^ 


0^ 




CO 

2 
























.S -(-s rv 





o 


^o 
























n. ^ >- 


O) 


*s 


a3 






















2 G^ 


ll. 




" 


CI. 
























% 


























g^a 































































A 


























03 ^ 




r' 


























P-X CD 




o . 


g 
























9 -S 






o 




























O) ' 


?- 
























j_, 




Si^ 


O 





























•=:'« 






























S o 


^^ 
























03 




©.a . 


2 
























.a 




2li 


CD 



.a 






















5i 




||2 




li 






















-^ 


































o 'S 


'T3 


1 — 1 






















3 '^ 




"o 


c3 


























(S""'^ 


<1 
























-^ 




q3 
S 


S 
^ 
























1 





80 



URINE ANALYSIS. 



O 



^bJD CD 

O g p 

(D O ^ 

o ^ +^ 

^ ^^ 

<D > O) 

^ ^ g 

g ^ a 



5-S 



3 QC 



-t:; rd '^ 






a; 



cj 



a a; 5 O) 



s 

-^ I- «^ 8 s S 

-^ O" 02 1^ an 03 03 

^ 9 c. " 



i^ ;;^ o 



<i^ fl s 
^ 03:3 



OQ " 



S 9 n 

^s a 

CD cj i; a> 



o^ ago; 



O) O 
1=1 " 

O ,~s 



02 

O c3 03 






fas ^^' 



OJ 



p 

05^ 



■4-" i, I 1 

Q f? C3 

-d ;=i ft, 

G ^ 0. 



ci 
o o 

O c. • 



a> o) ^^ 

f_, c. oS 

03 bJ2 i; 

(D^ CD 

a 

fT (D (D 



= a5:§Sl 

CDm ^ S OS 

3 






OQ D 02 



g.^--3 02 3 „ 
^ (D K* CJ 1^ 

^ o3 <D n, '^ a; 



ill 

-fa 



<D w 
=3 - 



O; CD 



ir CD 



CD ^TJ.S 03 




'ft 
o 
o 

OD 

o 

o fij 
•3 o 

wa 



o 

"I 

•?1 fl 



ft 



THE URINE CONSTITUENTS. 81 



«3 ^a^o5-g"3 ■S-^'SS -302 ^^ l» s§-=s«Js§ 

■§.§ ^lisiiiiiil :ip-,|i|s|r|ii;J| 
illi:i|tlii i P ^immU^t H!Si ^ 

lllWIiilllpI I ^1 I illf '|rr':l I 

: i-^ ill J ii_-^|| i 1%; : 4-s^-s i^i lE^ is| 

■+^ CD 






Q O 



03 

g.a 

« o 

<1 



o t2 

gS£ a 

a ^ * .2 



r2 ■ ^ 

.3 A 





S 




<D 




PI 




•rs 













<l 


O) 




,i4 


0) 


r— 1 









a 




a 


P 


S 


!3Q 



82 



URINE ANALYSIS. 



O 




^ ID 

Is 



m 



ft CD 



CD y^l^ 



13 o 
> Q 



cS CD 



<D CD 



CD 


-< 


fl 


^ 














■ , -1 


CD 


d 


-t-' 






r/> 








.2 


CD 


CD 


d 




-u 








d 


O 


^ 


-r1 




D 


>% 


CD 


f3 




ft 




S 


o 




>. 


2 


^ 


^ 


>, 




o 


.7) 


c3 


CD 


c3 


o 


03 




i=l 




o 


O) 


■O 


■73 


c* 


^ 


CD 








o^ 


cS 


D 




&c 








ce cD=+H 

ri CO O 



Ol 



r^ O 






^ o ?? 



^ O J^ 
CD -43 '-^'3 

cS ^ D 2 



•rH sn CD (^ 

rj 2 s &^v^ 



r-H a; 

c.a 



^3 ce 



CD 



CD so ^ 
■+J ft-(-i 



ft 



a 

O D 



^ a 



.1:! 5-, CD 



D O O) t3 

-o ft-t^-r; 



■CQ - c^_| ix; 
00 O O > 



C3 



11 
si 

D o 



bx; 



> CO 

^ 03 

D 

O 03 

§ «^ S 
^ 2 D 

oca -i:s 



a ^. 

o 
m D 



*5jo $c 



<!-2 a^^ 



■^ > ^ J_ 



^^ ft?? 

=^ _2^ CD 
O CD c3^ 

D D rrt 'S 
C^rd rrt CD 

03 'tS^ ^ 
ft^ <^ 



D (D 

1:^ ft 
03 






03 t, o3 o3 ^ 



o ^ ^ 

'^ o3 '-3 CD 

S D 
O ^ 

o3 d O .S bt.'?^ 



fl DQ CQ rt 
^. <1^ C ii 



b£- 



72 ?- b£^ 5 bt 



-T^ bi) q:> ->^ 



D 



CD d a CD O ^ iB 
-*-; CD <D -^ T ^ 

.a x^ ad--^ 



^ D 

CD r-. . 



D p Ti 



O S 



dH § 
'^ r,; ^ 

52 ^ ^ ^• 

<^ t» 03 rC 

c3 D CO 

^^?^ 

ftc3 ^- O 

ft <^ a ^ 
000 



o " o 
•^ a; C 



c3 
1^ CD 






c3 
O 
N 
O 

"ol 

a 

iH 
O) 
ft 

02 






THE URIXE CONSTITUENTS. 



83 



^ -r 




C ''-^ 


1 


^ 


^ 


, 




r—> 1 
































































'— '% 




'-"' T^ 


^ 


r^ 


>^ 


— ; 




2 
























?^ if s 




" "Z 


^ 


_~ 


c;, 


"" 




r^ S 












































^, 'Jl ■*^ 




•r! X 




>' 




OJ 




J- -r 




















t^ ^ 




.S 2 t^ 




ct -^ 


s- 




a; 


~ 








^ ^ c 




>■. S 


2 


c; 


o 


'o 




^3 




^ --J ~ 




5 X 




J 


2 


X 


s 


r~; 




"■ ~ S 




C '^ 


^ 




o 


.5 


■72 


-^ X 




>."^ --~i 




"^ ^ 




X 


^ 


r; 





B '^ 




















j_ 




5 ^'3 




^ — 




i^ 


^ 


^ 


>> 


rr CD 








C" r^ 


^ 


— ' 


'^ 


o 








"^ — X 




















b X S 




5".o 


-J 


>- 


^ 




"^ 


2 "^ 






^-r- 


X 


f- 


-*-' 


— ^ 


^ 


Iw 1-7-^ 




1^1 




^ X 

1^1 


X 


h3 


> 


r^ 


5 






" ;_-^ - 




■" HH 


s 


X 


> 


1^ 


-^ 


^ s 








5 ^£ 


X 




^ 


o 


ft 


























^=1 
|35 




X E 

2 3 


1 


-t-T 


X 


^ 


X 




ill 




^ " X 






^ 


^ 


. 


w 


.2 


H 3 — 




O '^ 








































c^ ~ 





w 


•■' 


■-' 


•"^ 


~- 


'— 


.^ >^ 




UJSl 


p 


a> 












£|-- 


g 


_— 5-< 


^ 














;z:!_>> 


5-1 


'T; 'tr y 


^ 


-^ 












•^ O) ri 


2 


•i 5 '^ 


^ 


.2 












S ^ 


1 


















C f5 W) 






£X) 


1 












a 


sii • r7^ 


5 














2^5§ 


V^ 


.— 5 ^ 


"3 


^ 'Z. 












u G-5 


d 




"c 


• '— c 












•S.2'^- 


CS 




































-* -1^ 




:i Q' 


— ^ 


^ ^ 












CS ^ 


^ X 


>.G -^ 




5 >. ^ 












>. = .=: 


II 


^•^ O 


X 


2 ^"2 














•ells 
und 

1 to 






















Jl 


2 


^ 








ZJ X 

9 1 






















•^ o 




3 ^ 


^ 


^ 








o3 




."■' Ci o 




;::^ 


S 


;::; 








S s 




-~3 


J-h" 

2 


■^ X 

_>.'2 




X 








■p 2 




X ^ ^- 


o 


111 

P SCO 


5 

X 


X 






^2 




















^ 




^ X 


o 


." 


c; 


3m 


Cu 


























i- 





























































ce 




















?-. . 




















II 




















l^ 




, '. 




r— • 












n-! 1-!^ 




















__, 




















.-. '73 
























<: 




-< 












<; 




jc' 








































—^ 
















. 
























'-' 




X 












"?^ 






















X 
















a> 




















-tj 




5 




o 














C3 




>■ 




r^ 












Ph 





84 



URINE ANALYSIS. 



OQ CO O rt 



5h _, l; M . 

o^-S go 

cc S cj o.'- 






I? CO OQ CQ 

o c 2 -^S 



CD 



P d o fl 9 

^^ a d^ 

jj jd '^ 



c3 d rt o 
CO O d 







i^ " 1^ 

^ 2 fl 

0^ =^ Cj 

d_g CD 



>.o 



d ^ d--^ 

d 2 05 c^ 

o fl d o) 

H H-j d 

^ d ^ Oi 

o ^^ -d 

^ ^ d 
OS 



^ d 

05 ■> 



d >. 

II 

O ci 

5h -tJ 






OS OQ'+H 
(D O 

• rH P ao 



•d^ d 



5h r-H n; .r-l C^ 

^ d > at^ 

^ Je 03 ^ t^, 

"^ CD CD C' 



2 ft^ 

OS J^'d 



d 5.2 



CO 



^ >i 



a 






'. CO 

CO CO 
«0 CC 



.., d o 



.^ "S^ 



E^ cs 



d o 



CD 



d 






d 



S =* 

•^ m 



<X> 



cD'Td'^k: 
c!^ ^ d . 



d o) 



S g o ^ c o 
"^-.o cs d 

d ce o os d 



IK d 
CO o 

d " 



CD 

O) 
O 

ft OS 

d t:^ 

oS o 
ft O O) 

cS g 

03 (j; > , 



° (D 

>>d 

d3i 

<D 5^ CO 



■D cS 



OS 



jd d -^ 
cS OS 



CD O 

^ o 

0) 

d>: o^ 

o o o 



i^ 



r^^ O 
g§^ 



iT) C^ 
;- <D 



^ <^ d 

CD O ^ i^ 
U CD tJD <1^ 

O QO-d X5 



o 
d 

.2 
'o 
qd 


le spe 
is low 
or is 1 
there 


CD 


".^1s 


'oS 


cS > (D 



cS o 



o ft^^ a; 
cS oS st^ ft 



O K-i 



Sh O <D 



^•^ CD 

I— ' O (X) CO '^-' 

2 =* © ^Ti 

^ 0^ d 



<D cS <D '-^ 
^ ^ -d ^ 



d o 



.2 a^ ^ 

cd «2*Sr^5::; 
o CD ^^ O 

'^'H a ^ "^ 

*?H ■, 'd <D 

O ft O d 



d §-S^ 

^ ^ u 

^4iJ CD p 



<^ d i^ <D ^ 
^ OS d 



OQ 



g^ ^ :^ d 



d 

CD 
^ (33 



Q 



THE URINE CONSTITUENTS. 



85 



±: '^ -^'r^ 






lb 

oc 

o 



;;: o 

oc ,ti 



P 02 Ci ^* oc CO '^ 
.^ -r-i '^ >^ (D q^ <D 

grnkric; a)5(D-^a3cocj2 
a.- G 5 ,- .i^ oc OS 1^ o o :- 



OD o =- '^ -- 



X ^ > o C i£ '-' 

-- C SS ^ »2 S 



1J.!^ n. -^--^ y-^ 



^ 2 
O^ 



03- 



O^ 



r/1 




o 


c5 




0) 


o 




















o 


o 




p 


S-i 


?^ 


CC 





oc 






03 CO 

03 

rt 9 



8g 



6 q3 i a 03 

-^ fl ^ 03 5^ 

o 'P I - 2 

- "t^ oc P CO 
•o TiJ CO -r 

03 rj c5 -1-=' 
■p <^^ 
O 03 02 • -*^ 

.E -- 03 >j 

■ P O 

^•^ S^ 

-P OS 



h-H P 



P-r -P 

o r -^ 



oi 

5- .P '^ ^ 






CO > 



O 
O 



03 CO -1 O ^ 
pa: 



15" • i ^'^^ ^ 

S-S 03,^^ g o-S o^ o^ :^^\c 03 ,^,^ P 

cP'-c3'^-:=;'^-2-'^ 
o cr' P .^ 03 ^ ''3 cc 03 



„ — . 0, o ' _ , 



"' X 0.2 =3 p 03^ 
.Sp;£p"o5S 
Sa)^^^^=5O03 

H-! .P ^ O rt £ 03 o 



SH p5 





^ii 










^ +3 T^ ■"" 




P OQ 






i> i 


.p a 




excess 
can be 
titative 




CO 

P 0) 
O.P 






ced on 

and if 

water, 

turbid 

rbonate 




X o 

<^ ^ 
"Z JO 

S 03 








amnion 

>itate is 

a m m 




p oc a 




'-^ "C 






P ^ Orr- C3 




S o 






r^- 




^-2 p 

03 2 CT' 




5 p 






"5^ p ^ " 

O-r' -P 5- 








^i>B.s 






•Sl^ 














^ s^ 


03 




r there b 
of phospl 
only by a 




-^ 5-1 

CO a 

O o 








2-p 


s 




-M Cvi OQ 5- ^ 






03^ 






cence 
•f acet 

ssed ii 
L be r 
[)itatio] 




■^ P 

03 33 
1^ 


_p 




Ii 

02.2 


solnti 
, The 
s sol V 




Wliethe 
ificiency 
rtained ( 


02 


p'o 

C-03 
-1| 






Efferves 
Idition c 
.s be pa 
tter will 
e preci 


s 


^ 

03 


'bi 
i 

OQ 




PrH 

^ OQ 

0£ 


rom acid 
a rbonate. 
ected, di 




<33 03. 










^' 03 ^ ^ 


03 




li 




.P 




t: o 


03 


P 






zi b£p^ -tJ 


O 


• 1-^ 


+J 




— ' 


•-^j -^ .—1 


5-fe 

P ^ 

^:p 

li 

„ o 

•^ 03 


V-.-^ 0) 


03 


p o 


Tjd 




^ O CO' >, '^ 




s s 




_o 


P 2 


R o-P 


low. 

No characteri 
effect ni)on t 
physical prop 


P 
03 

O 
oc 
03 

^3 


^ oc 
"P CO , 

03 ^ 

'Z s 


_CC' 

CO 

03 

"&. 
CO 


s 

'o 

03 


There is alw 
a deposit in ni 
which coutai 
carbonates if ; 
appreciable qu 


tity IS present. 
Urine contt 
in o- these const 


a 

O' 

_^ 
5 




_o 


' ' 

03 P 
P"X3 

^ 

V. if' 
03 P 
^ 'P 

c3 


a sweet briar od 
when deconip 
tion sets in, hy( 




c3 




^ o 


_aa 


'^ 


>> 




c3 






'^ 






u 




+^ 










^ 






S^ 










•rH aQ 


CO 


"o 


■—1 ^ 




■^ 












03 6 
P.P 




^ oc 
03 

O o 


03 


>» 


oe ce 




03 03 

P P 






S 03 






—^ CO 




.P X 

S, 03 






















•^^ 




"^ 


03 


o ? 




•g^ 






•5 5 






^ 03 




h^ 


-^ 




O p 




-3^ 03 






<1 05 






^ 






^ 


03 






;m 






!-( 






O 




s 


OC 


be 


s 

















CQ 






86 



URINE ANALYSTS. 



^ a:" ^ CD 



^ 


o 


O' 




^H 


O) 


S (» 


■ ^ 


ft O; 


CS 












CD 



13 oj f- " 



^ ^ S o 

t^_^ CO ,12 ■+J 



O CD 



W CD • r- 






CD 
9 tB 



CD S 

> O) c; ct 



05 a: 



^ ft 
o5 



^ >.'-^ 



o^ 



^ (D 
O fK 

£ I 



oil ' 

o s ^ 

•p bc o K 

= ?<« 

■ " — ' O CD 



■CD O 

r-3 ~' 



S ^ fl J^ _r-l 



-S 






O .;^ -*J ^ :X r-2 




o3 



05 .G 

r^ 05 



3:s - ^ 



^ Oj-r3 o 



^ o 

G 5H 

biDtl 



O 05 

o ^ 



3^ 



■'^, 'ft 
orG 



O G 

G "3- 
0^ ^ 
-^^ G 

OjO 

^^ 



-<:^ 



^'^ Gr^-'r 



>, CD 



•M-l CC rG 



brj o 

"5 CD 



,2 b 



^P§ 



O--^ f-, G 



H P ^ 



05 CD 
'S3 



^ X 

Ci CD 
CD ^ 



X..2 
2''^ 3 

^ 5 G 



G .^ 



■ so I Oj >, 

•S3 o^^ 

c o o f^ G 
■^ '^ o. G o 

^ 05 C ^ 

g'23 -^ S 
.^ ;r; oi— I f-i 

fn G 0^ Tj 

^ bJj o ,^* o 

G G ~^ 



O 05 




a; jh 




r~, 1 


. 










is 


2 
'a 


ojp 


CD 



CD rO O 



oS 05 
2 8 

Tx) oi 






CS 



05 05 



^ ? "3 05 
^ ^'^:^ 05 . 
O r- ?H CD 



■|^ 






W 



rft .2 

O r-3 



THE URINE CONSTITUENTS. 87 



|5-c =|-oi-o|.|i2 .= 

x " ;- i; -r-. r- ^ I' >i cv ^ G Hj 



' ~ ^ ^ 50 O " SB^^ 



® =c >>iC ■72 .^ •? c .-^;^ ." fl 







%. 


"3 


o ^ ^ 


::_ 


'- 


•-z: ov 


^ 


O 


CS OD P^ 














r^ 


::: 








- cu ;=. 


:^ 


X 


sH ;ri P-i 


x 










-t^ 


' ' 


^z .== 


'J2 


o> 






^ 


"5 5C ^ 


<D 














^ 


T 


- bJO == 


~ 


Qj 


t;-^ 2 






H 


"^ 





'x 5 




" 


X -^ ^ ^ -" 


^■"3 




•| 


..-^^l 






-M 




>H 


:? CD CD a, 


>-. ^ 


.2 


U 


K X -73 02 

c3 ;^ 


.2 ^ 


low speci 
ity. 
Urine 


1?& 







5 CD =« 2 X 



.. ^ J- <^"B'7 - — i; "^ ^ ■^ "^ ^ "^ -^ ~ xf ' S 












^ „ „ ^^ r- - o ::^'Z 2 '^ '^ ^ '^.z: -^ ^ 






1 


CD 
> 


.9 




i£ 


3 


o 






• 1— 1 






-f^ 






o 






c^ 






,—1 






^ 






S-i 






£ 


'o 





OS 



88 



URINE ANALYSIS. 



Pathological Indications. 


&J0 

.s 
1 

a 
o 

'ft 

a, g 
^2 

O 


Chemical Tests. 


bath. Add water and again evapo- 
rate on the bath. The residue is par- 
alactic acid and the various salts may 
be prepared as directed. 

Place some of the urine in a small 
beaker or flask, and cover with pa- 
per moistened with lead acetate and 
gently warm when the paper will be 
blackened. 


Influence of the con- 
stituent upon the 
physical properties 
of the urine. 


Arises from de- 
composition of sul- 
p h u r containing 
organic bodies. 


Reaction of the 
urine in which 
the substance 
occurs. 


'o . 

^ <^ 

'S.5 

II 

O 


6 


Sh ft 



ttt» tl Mttsii. 



€^^ 



€1^1 /^e degj/u-eif €>. 



^Ijns'ual anb Cbemical Character; 



fjt/^-^ {LJa.€^4^ 



'eccci-c^-T^ 



^^^ €Z'/2Mea''t= 



i^'^i^e 



4-ci-led 



(?^- (?^ 

^7 



€?^d'AA^(^t^fed -^ ^-(^(^4- 



M^'T^yi^^n 



glkroscopital €,t-ammalion. 



90 URINE ANALYSIS. 



^atl^o^ita' Inbi^atioiTS. 



^ (4^c.t€J... 



THE URINE CONSTITUENTS. 



91 



/ 














Fig. 2. 




Fig. 1. Sediment in Acid Urine.— Calcium oxalate, uric acid, and amorphous 
acid urates. (Nkubauer and Vogei..) 

Fig. 2. Sediment in Alkaline Urine.— Triple and amorphous phosphates, 
ammonium urate and bacteria. (Neubauer and Vogel.) 



DM 



URINE ANALYSIS. 





Fig. 15. Forms of Uric Acid. (Schotten.) 

Fig. i. Leucin balls on the left— Tyrosin needles on the right. (Neubaueii 
and VoGEi..) ' .. ■ ■ ' 



THE URINE CONSTITUENTS. 



m 



Fig. 5 




Fig, 6. 




Fig. 5. Cystin. (Neubauer and Vogel. 
Fig. 6, Cholesterin. (Harley.) 



94 



URINE ANALYSIS. 



Fig.t 




Fitf.8 




FiO, 7. Forms of Calcium Oxalate, (v. Jaksch ) 
Fjg. 8. Forms of Calcium Carbonate. (Vaughan.) 



THE URINK CONSTITUENTS. 



96 



Fi^ 9 




Fig. 10. 




Fig. 9 Ammonium Magnesium (Triple) Phosphate, (v. Jaksch.) 

Fig. 10. Forms of Casts, a— granular cast; &— the same beset with renal 
epithelium; c-the same with colorless blood cells; d-the same 
with drops o^ fat and tatty crystals; e— hyaline cast covered with 
red blood cells; /-the same with renal eithelium; .g— east of white 
blood cells, (v. Jaksch.) 



9() 



URINE ANALYSIS, 



Fig. 11 




Fig. 11. Cylindroids from the urine in congested kidney, (v. Jaksch. 



THK URINK CONSTITUKNTS. 



97 



Fig. 12. 




Fig. 12. a— Spei^matozoa; 6— Red blood cells, some crenated; c— Pus cor- 
puscles. (ScHOTTEX, Nefbaur and Vogel.) 



98. 



URINE ANALYSIS. 



Fig.13. 




yr^U 




Fig 1. '5. a— Micrococci ; b — Bacilli; c — Filaments of moulds; d — Yeast-cells; 
e— Micrococcus ureae. (v. Jaksch.) 

F'kj. 14. a — Squamous epithelium^; b — Epithelium from the bladder; e— Epi- 
thelium from the kidneys; d— Fatty epithelium from the kidneys. 
(v. Jaksch.) 



THE URINE CONSTITUENTS. 



99 



Fig. 15. 




Fig. 15. Absorbtion spectra (after Ha3IMARsten) : — 1. A solution of oxy- 
hfemoglobin; 2. A solution of haemoglobin, obtained by treating 
oxy-hfemoglobin witli an ammoniacal ferro- tartrate solution 
(Stokes' fluid). :>. A weak alkaline solution of methsemoglobin. 
4. An alkaline solution of heematin. 5. An alkaline solution of 
hfemochromogen, obtained by treating an alkaline hsematin solu- 
tion with Stokes' fluid. 6. An acid solution of urobilin. 



INDEX. 



Acetone 36 

Acetacetic Acid 36 

Acidity 52 

Adamkiewicz's reaction.-l 39 

Albumin 39, 64, 66 

Albuminoids 38 

Albumose 40, 67 

Alkalinity 52 

Allantoic acid 20 

Allantoin 19 

Allanturie acid 20 

Alloxan 18 

Alloxantin 17 

Almen's test 43 

Amido acids 32 

Ammonium Magnesium phos- 
phate 35 

Ammonium purpurate— — 16 

Benzoic acid 26 

Benzoyl chloride test 9 

Bile 44 

Biuret 10,39 

Bioxam's test 10 

Bottger's test 46 

Cadaverine SS 

Calcium oxalate 27 

Calcium phosphates 35 

Calcium sulphate 27 

Chlorides 53 

Cholesterin 36 



Composition of urine 69,70 

Creatinine 21 

Cyanuric acid 17 

Cystin 32 

Czapek's method 64 

Densimetric method 65 

Donne's test 44 

Empirical solutions 49 

Esbach's albuminometer 66 

Ether, sulphuric acids 27 

Fats 37 

Fehling's test 46 

Fehling's solution 57 

Fermentation test 47 

Fibrin 43 

Fixed alkali 12 

Furfurol test 9 

Globulin 40, 64, 66 

Glycocoll 26 

Gmelin's test 45 

Grape Sugar 46,57 

Guaiac test 43 

Hfemoglobin 42 

Hammarsten's method 66 

Haycraft's method 64 

Heintz's method 62 

Heller's test 40, 43, 46 



102 



IIR1>;E ANAIASIS. 



Hippurie acid 

Hoflfniann's reaction. 
Hofraeister's method. 

Huppert's reaction 

Hiifnei''s metliod - 

Hydantoic acid 

Hydroquinone 

Hyposuipiiurous acid . 

Indican 

Tndigogen 

Indol . 

Indoxyl 

Iodoform test 



Jaffe's test 



Konigand Kiscli's method. 
Kiihne's peptone 



Leucin 

Lieben's test 

Liebermann's reaction 

Liebig's method 

Ludwig's method 



Magnesia mixture-^ 

Magnesium ammonium ph( 

phate 

Maixner's method 

Melting point 

Methsemoglobin 

Miilon's reagent 

Mohr's method 

Moore-HeUer's test 

Mucin-like substance 

Murexide test 



Neutral sulphur 

Nitrogen, estimation 
Nylander's test 



30 



42 



6:1 



35 



24 


Oxalic acid 


27 


34 






41 


Parabanic acid 


20 


45 


Peptones 


41,67 


61 


Pettenkofer's test 


44 


-m 


Phenol 


29 


82 


Phenol-sulphuric acid 


28 


28 


Phenyl-hydrazine test 


46 




Phosphoric acid 


.___- 34, 56 


3U 


Piria's reaction 


34 


30 


Pohl's method 


67 


30 


Proteids, classification 


37 


30 


Pus 


43,44 


3B 


Putrescine . _ . _ 


33 




Pyroeatcchin -.. 


31 



Quantitative analysis 
Quantity of urine 



Robert's-StolnikofT's method. 

Scherer's method 

Scherer's test 

Skatol 

Skatoxyl 

Solids, total 

.Speci tfc gravi t y 

Standard solutions 

Sulphuric acid 



33, 



27, 



Triple phosphate, 
Trommer's test- - 
Tyrosin 



Urea 5, 

Uric acid 12, 

Urine, composition of 69. 



Volatile alkali 

Volhard's method. 



Xanthine compounds. 



